1. Explain how the solubility curve lab works.
- In the lab we will be collecting data to make a solubility curve for succinic acid. The lab shows how to use properties of a saturated solution, investigating solvent temperatures, and then repeat the data to be sure.
Sunday, June 30, 2013
Homework #10
Questions #9-27, 33, 35
9. .2 x 55= 11
55 - 11= 44
10. 15,000
11. Polar molecules are partially negative and positive so a water molecule (having a V-shape) has one oxygen end (which is negative) and two hydrogen ends (which are negative).
12.
13. A. K+ ion: oxygen (negative) end
B. Br- ion: hydrogen (positive) ends
15. They include damage to to the nervous system, brain, kidneys and liver, which can even lead to death. They also bind to proteins and prevent them from performing their normal tasks.
16. A. Lead: people get water through lead water pipes connecting to households (but cause lead poisoning). And they also have lead cooking vessels.
B. Mercury: it's an electrical conductor and used as thermometers.
17. Hydroxide
18. Hydrogen
19. A. Base
B. Base
C. Acid
D. Neutral
20. A. Soft drink
B. Black coffee
C. Milk of magnesia
21. 2.0 more times acidic.
22. 1. When pH is too low in rivers, lakes, or streams, fish-egg development is impaired causing hampering the ability of fish to reproduce.
2. Bodies of water with low pH values tend to increase the concentrations of metal ions in natural waters by leaching metal ions from surrounding soil, which are toxic.
3. High pH is a problem for living organisms because alkaline solutions are able to dissolve organic materials, including skin, and scales.
23. Polar molecules tend to dissolve readily in polar solvents, but nonpolar liquids are good solvents for nonpolar molecules.
24. Lamp oil because oils readily dissolve in nonpolar body oils.
25. Oil cannot separate causing the salt not to separate. Water on the other hand is polar, so the salt can dissolve.
26. A rule that tells why polar substances dissolve in polar solvents and nonpolar substances dissolve in nonpolar substances. It also tells why nonpolar liquids are usually ineffective in dissolving ionic and polar molecular substances.
27. Water and grease don't mix together well, so soap is needed to clean the grease.
33. A. Nonpolar substances
B. There are other chemicals in the cleaner that can clean hands for thoroughly than water.
35. Hydrogen because hydrogen has a +1 charge, while Fluorine has a -1 charge.
Thursday, June 27, 2013
Quick Blog Question
Explain how to do solution concentration problems? What is the tricky part?
- To do solution concentration problems you first add the grams of the elements or compounds (like NaCl) and then the number of grams in the water. Next, you have do percent by mass. You now take the mass of solute and divide it by the mass of solution. Next, you multiply it by 100 to get your percentage. The tricky part is calculating the percent of mass.
- To do solution concentration problems you first add the grams of the elements or compounds (like NaCl) and then the number of grams in the water. Next, you have do percent by mass. You now take the mass of solute and divide it by the mass of solution. Next, you multiply it by 100 to get your percentage. The tricky part is calculating the percent of mass.
Homework due Friday July, 28th
1. A. You would lose potassium chloride due to the temperature change.
B. 
2. A.
B. i.
ii. 20g
3. A & B.
C. The precipitate is double because I added more water making it less concentrated.
Test #2 Semester 1 Review
Answer the following questions:
1. Define pH and give examples of an acid, a neutral substance and a base. What pH number will each of these substances have?
- pH is an acidic scale.
- Examples: 1 neutral substance: water 7
1 acid: vinegar 1
1 base: ammonia 9
(helpful pages 68-70)
2. The speed limit in Canada is 100 km/hr. Convert this to meters/second?
- 360,000,000 meters/second (you get 100,00 which is meters per hour now change it to second so multiply by 60 twice and get your answer!)
(helpful pages see sheet on unit conversion)
3. How many decimal places change when you convert 905 mg to kg? What is the answer?
- 6 decimal places change
- .000905 kg
(helpful pages see sheet on unit conversion)
4. What are the charges and weights of electrons, protons, and neutrons?
- Electrons: -1 (negatively); barely weigh anything
- Protons: +1 (positively); 1 atomic unit
- Neutrons: Neutral 0; 1 atomic unit
(helpful pages see page 38)
5. What is positive, an anion or cation? How is it formed?
- Cation; formed when an element loses an electron.
(helpful pages see page 39)
6. The first column on the periodic table (Na, K, Rb) tend to gain or lose how many electrons and have what charge?
- Lose 1 electron to get a +1 charge
(page 40)
7. The second column on the periodic table (Mg, Ca, Sr) tend to gain or lose how many electrons and have what charge?
- Lose 2 to get a +2 charge.
(page 40)
8. The sixth column on the periodic table (O, S, Se) tend to gain or lose how many electrons and have what charge?
- Gain 2 electrons to get a -2 charge.
(page 40)
9. The seventh column on the periodic table (F, Cl, Br) tend to gain or lose how many electrons and have what charge?
- Gain 1 electron to get a -1 charge.
(page 40)
10. The eighth column on the periodic table (He, Ne, Ar) tend to gain or lose how many electrons and have what charge?
- Don't gain or lose electrons; they are Noble Gases.
(look at the periodic table)
11. Explain and give examples of negative and positive ions?
- Cations and Anions; H+ and O-2
(see pages 39-40)
12. What is an atom compose of?
- Protons, neutrons, and electrons.
(common knowledge)
*molecule > atom > nucleus > proton/neutron > electron
13. Why can't water be 100% pure? What is in even the purest water?
- Impossible to obtain; too expensive; dissolved minerals and gases are always in even the purest water
(common knowledge or see last weeks test study guide)
14. How can we help dissolve more solute in water? (List several ways)
- Raise temperature; heating the water
- Under pressure
- Vigorously stirring; mixing
Example: a lot of CO2 is in coke; coke is under pressure because of the CO2
15. Explain how we know what ionic compounds and the subscripts are formed from K+ and I-. From Ba2+ and OH-. From Al3+ and O2-.
- Kl; Ba(OH)2; Al2O3
- Balancing them
(see Wednesday's quiz)
16. What is the atomic symbol for mercury? What is it's atomic number? Atomic weight? How many protons, neutrons and electrons does it have?
- Hg; 80; 200.59
*Note: atomic number is the top and the weight is the bottom
(see periodic table and page 34)
17. What is an unsaturated versus a saturated solution?
- Unsaturated solution is a solution that contains less dissolved solute than the amount the solvent can hold at a specific temperature while a saturated solution has as much dissolved solute that it can hold at a specific temperature.
(see pages 53-54)
18. Explain how to create a supersaturated solution. Explain the chemistry behind it.
- Unusual term; adding salt as we heat it and then we're cooling it down now that it has a lot of solute and for a short time we can keep a lot of solute in solution more than needed or expected at that lower temperature (unless we jiggle it; just touching it causes it out of solution/precipitate now only some solute is in solution and it goes back to normal).
19. Define the following terms (and explain the Chemistry concepts behind them).
A. Polarity
- When two opposites attract each other.
- Ex. H20-V shaped positive on the bottom end and negative at the top end
(see last tests study guide)
B. Ionic bonds versus covalent (molecular) bonds
- Ionic bonds connect ions and covalent bonds connect molecules. Ionic are not as strong.
NaCl separates in water Na goes to negative side and Cl goes to the other
C. Chemical reaction versus chemical reaction
- Teacher tired.
- Entail the breaking and forming of chemical bonds, causing atoms to become rearranged into new substances.
D. Reactants versus products
- Reactants are the original (starting) substances in a chemical reaction (written to the left of the arrow), while products are the new substance or substances formed from the rearrangement of the reactant atoms (written to the right of the arrow).
E. Solute vs. solvent vs. solution vs. solubility
- Solute is the dissolved substance (salt is an example)
- Solvent is the dissolving agent (water is an example)
- Solution is a homogeneous mixture of two or more substances
- Solubility is the max quantity of a substance that will dissolve in a certain quantity of water at a specified temperature in water.
F. Unsaturated vs. saturated vs. supersaturated
- Unsaturated: less solute
- Saturated: contains as much solute as possible in the temperature
- Supersaturated: unstable; too much solute
G. Mean vs. Median
- Mean is the average (adding up all data and then dividing)
- Median is the middle value
H. Chlorine vs. Chloride
- Chlorine is an element
- Chloride is an ion (when it gains an electron)
I. Hydrologic Cycle
- Water gets evaporated to vapor then goes to the the sky and gets precipitated then down back into the ocean. A cycle is a closed system so no water is created or destroyed.
J. Subscript vs. superscript
- Subscript is below the element/compound, superscript is above.
L. Tyndall effect
- The scattering of light indicated that small, solid particles were still in the water.
M. Catalyst
- Speeds up the reaction
N. Conservation of matter
- No matter is added or destroyed
20. Chlorine and ozone (O3) are added to water to kill what?
- Bacteria
21. How would you figure our which is proper ionic formula? McCl vs. MgCl2
- MgCl2 because Magnesium has +2 charge so Cl- needs 2.
(see Wednesday's quiz)
22. The acidity (or basic-ness) of a substance if measured by ...
- pH
23. How many protons are in each element?
- H: 1
- Mg: 12
- Na: 11
- Cl: 17
24. Explain undissolved solute at the bottom of a beaker of solution?
- The temperature was not high enough
- Not enough pressure
- It was saturated
25. Make up your own question and show it to a neighbor in the class! :)
Ex. Why does the temperature of the solution effect the solubility of the substances?
1. Define pH and give examples of an acid, a neutral substance and a base. What pH number will each of these substances have?
- pH is an acidic scale.
- Examples: 1 neutral substance: water 7
1 acid: vinegar 1
1 base: ammonia 9
(helpful pages 68-70)
2. The speed limit in Canada is 100 km/hr. Convert this to meters/second?
- 360,000,000 meters/second (you get 100,00 which is meters per hour now change it to second so multiply by 60 twice and get your answer!)
(helpful pages see sheet on unit conversion)
3. How many decimal places change when you convert 905 mg to kg? What is the answer?
- 6 decimal places change
- .000905 kg
(helpful pages see sheet on unit conversion)
4. What are the charges and weights of electrons, protons, and neutrons?
- Electrons: -1 (negatively); barely weigh anything
- Protons: +1 (positively); 1 atomic unit
- Neutrons: Neutral 0; 1 atomic unit
(helpful pages see page 38)
5. What is positive, an anion or cation? How is it formed?
- Cation; formed when an element loses an electron.
(helpful pages see page 39)
6. The first column on the periodic table (Na, K, Rb) tend to gain or lose how many electrons and have what charge?
- Lose 1 electron to get a +1 charge
(page 40)
7. The second column on the periodic table (Mg, Ca, Sr) tend to gain or lose how many electrons and have what charge?
- Lose 2 to get a +2 charge.
(page 40)
8. The sixth column on the periodic table (O, S, Se) tend to gain or lose how many electrons and have what charge?
- Gain 2 electrons to get a -2 charge.
(page 40)
9. The seventh column on the periodic table (F, Cl, Br) tend to gain or lose how many electrons and have what charge?
- Gain 1 electron to get a -1 charge.
(page 40)
10. The eighth column on the periodic table (He, Ne, Ar) tend to gain or lose how many electrons and have what charge?
- Don't gain or lose electrons; they are Noble Gases.
(look at the periodic table)
11. Explain and give examples of negative and positive ions?
- Cations and Anions; H+ and O-2
(see pages 39-40)
12. What is an atom compose of?
- Protons, neutrons, and electrons.
(common knowledge)
*molecule > atom > nucleus > proton/neutron > electron
13. Why can't water be 100% pure? What is in even the purest water?
- Impossible to obtain; too expensive; dissolved minerals and gases are always in even the purest water
(common knowledge or see last weeks test study guide)
14. How can we help dissolve more solute in water? (List several ways)
- Raise temperature; heating the water
- Under pressure
- Vigorously stirring; mixing
Example: a lot of CO2 is in coke; coke is under pressure because of the CO2
15. Explain how we know what ionic compounds and the subscripts are formed from K+ and I-. From Ba2+ and OH-. From Al3+ and O2-.
- Kl; Ba(OH)2; Al2O3
- Balancing them
(see Wednesday's quiz)
16. What is the atomic symbol for mercury? What is it's atomic number? Atomic weight? How many protons, neutrons and electrons does it have?
- Hg; 80; 200.59
*Note: atomic number is the top and the weight is the bottom
(see periodic table and page 34)
17. What is an unsaturated versus a saturated solution?
- Unsaturated solution is a solution that contains less dissolved solute than the amount the solvent can hold at a specific temperature while a saturated solution has as much dissolved solute that it can hold at a specific temperature.
(see pages 53-54)
18. Explain how to create a supersaturated solution. Explain the chemistry behind it.
- Unusual term; adding salt as we heat it and then we're cooling it down now that it has a lot of solute and for a short time we can keep a lot of solute in solution more than needed or expected at that lower temperature (unless we jiggle it; just touching it causes it out of solution/precipitate now only some solute is in solution and it goes back to normal).
19. Define the following terms (and explain the Chemistry concepts behind them).
A. Polarity
- When two opposites attract each other.
- Ex. H20-V shaped positive on the bottom end and negative at the top end
(see last tests study guide)
B. Ionic bonds versus covalent (molecular) bonds
- Ionic bonds connect ions and covalent bonds connect molecules. Ionic are not as strong.
NaCl separates in water Na goes to negative side and Cl goes to the other
C. Chemical reaction versus chemical reaction
- Teacher tired.
- Entail the breaking and forming of chemical bonds, causing atoms to become rearranged into new substances.
D. Reactants versus products
- Reactants are the original (starting) substances in a chemical reaction (written to the left of the arrow), while products are the new substance or substances formed from the rearrangement of the reactant atoms (written to the right of the arrow).
E. Solute vs. solvent vs. solution vs. solubility
- Solute is the dissolved substance (salt is an example)
- Solvent is the dissolving agent (water is an example)
- Solution is a homogeneous mixture of two or more substances
- Solubility is the max quantity of a substance that will dissolve in a certain quantity of water at a specified temperature in water.
F. Unsaturated vs. saturated vs. supersaturated
- Unsaturated: less solute
- Saturated: contains as much solute as possible in the temperature
- Supersaturated: unstable; too much solute
G. Mean vs. Median
- Mean is the average (adding up all data and then dividing)
- Median is the middle value
H. Chlorine vs. Chloride
- Chlorine is an element
- Chloride is an ion (when it gains an electron)
I. Hydrologic Cycle
- Water gets evaporated to vapor then goes to the the sky and gets precipitated then down back into the ocean. A cycle is a closed system so no water is created or destroyed.
J. Subscript vs. superscript
- Subscript is below the element/compound, superscript is above.
L. Tyndall effect
- The scattering of light indicated that small, solid particles were still in the water.
M. Catalyst
- Speeds up the reaction
N. Conservation of matter
- No matter is added or destroyed
20. Chlorine and ozone (O3) are added to water to kill what?
- Bacteria
21. How would you figure our which is proper ionic formula? McCl vs. MgCl2
- MgCl2 because Magnesium has +2 charge so Cl- needs 2.
(see Wednesday's quiz)
22. The acidity (or basic-ness) of a substance if measured by ...
- pH
23. How many protons are in each element?
- H: 1
- Mg: 12
- Na: 11
- Cl: 17
24. Explain undissolved solute at the bottom of a beaker of solution?
- The temperature was not high enough
- Not enough pressure
- It was saturated
25. Make up your own question and show it to a neighbor in the class! :)
Ex. Why does the temperature of the solution effect the solubility of the substances?
Wednesday, June 26, 2013
Sam Phillips - My Career in Chemistry (Live SF edit)
This is a cute chemistry song I thought would be fun to post! Enjoy! :)
Check out more Sam Phillips at https://www.facebook.com/SamPhillipsMusic?ref=ts&fref=ts
Quiz Thursday 27
Part 1: Terms
1. Saturated
- Undissolved as a solid on the bottom of a container, no matter how long you vigorously stir.
2. Solubility
- The maximum quantity of a substance that will dissolve in a certain quantity of water at a specified temperature. Example: 100 g.
3. Unsaturated Solution
- A solution that contains less dissolved solute than the amount that the solvent can normally hold at that temperature.
4. Supersaturated:
- An unstable solution that contains more solute than could usually be dissolved at that temperature.
Part 2: Understanding
1. Understand constructing a solubility curve and be able to explain it.
- The graphical representation of the relationship between solute solubility in water and temperature.
2. Sugar dissolving in hot tea but not cold.
-It will dissolve in hot tea because the temperature can dissolve more of the solute the higher it is. The higher temperature causes an unsaturated solution
Explain your way of solving math word problems when answering solubility questions:
I usually look at how they set up the problems in the sample questions and try to solve it the way the book does (usually with proportions or by looking at the graph).
Homework #8 Semester 1
1-3 on pg. 56
1. A. 106 grams
B. 45 grams
2. A. 45 grams
B. 20 grams
3. A. 75 grams
B. 90 grams
1-8 on pg. 82
1. Sugar cubes dissolve in tea (tea being the solvent and sugar the solute). The reason it dissolves completely in hot tea instead of iced tea is because the sugar dissolves faster in the hot tea and slower in the iced tea (the molecules move slower).
- The differences in temps can effect the solubility.
2. 48 grams.
3. A. 50 200g
B. 177.5 710g
C. 473 1892g
4. A. Least soluble: potassium nitrate
Most soluble: potassium chloride
- NaCl, KCl, KNO3
B. Least soluble: potassium chloride
Most soluble: potassium nitrate
- KNO3, KCl, NaCl
5. Saturated is when something can be soaked thoroughly while unsaturated is a solution contains less dissolved solute than the amount that the solvent can normally hold at that temperature.
6. A. 32
B. Supersaturated saturated
C. 70 90g
7. A. nothing the crystals will dissolve
B. precipitate a little the crystal will form at the bottom
C. precipitate a lot the crystal will will add to the precipitate at the bottom
8. 23%
1. A. 106 grams
B. 45 grams
2. A. 45 grams
B. 20 grams
3. A. 75 grams
B. 90 grams
1-8 on pg. 82
1. Sugar cubes dissolve in tea (tea being the solvent and sugar the solute). The reason it dissolves completely in hot tea instead of iced tea is because the sugar dissolves faster in the hot tea and slower in the iced tea (the molecules move slower).
- The differences in temps can effect the solubility.
2. 48 grams.
3. A. 50 200g
B. 177.5 710g
C. 473 1892g
4. A. Least soluble: potassium nitrate
Most soluble: potassium chloride
- NaCl, KCl, KNO3
B. Least soluble: potassium chloride
Most soluble: potassium nitrate
- KNO3, KCl, NaCl
5. Saturated is when something can be soaked thoroughly while unsaturated is a solution contains less dissolved solute than the amount that the solvent can normally hold at that temperature.
6. A. 32
B. Supersaturated saturated
C. 70 90g
7. A. nothing the crystals will dissolve
B. precipitate a little the crystal will form at the bottom
C. precipitate a lot the crystal will will add to the precipitate at the bottom
8. 23%
Tuesday, June 25, 2013
Extra Notes on Water Testing Lab
Quiz #7
~We conducted a confirming test and a qualitative test.
~What did we look at in the confirming test: change in solution color or for the appearance of a precipitate
~ Precipitate: Insoluble material
~ Qualitative Test: absence or presence
~ Quantitative Test: amount
~Anions and cations are found in groundwater and tap water
~ Blank: no ion to see if the others have ions
~ Reference Solution: comparison; solution of known composition
~Compare with blank to see if substances have ions.
New Blog Question
What did you learn from this lab about water and about process?
- I learned that distilled water's image can be morphed just by mixing with a simple substance (KSCN for example). I learned that (about process) a lot of steps were needed for this experiment which in my mind I thought would be simple and quick. It was very interesting to see the results of adding the substances to the water and I really enjoyed this experiment! :)
Quiz Questions #7
1. Pure vs. Impure water, why can't we confirm absence of an ion?
- The reaction when adding a substance to the mixture causes the ion to be so small to the naked eye. So it's impossible to say that there is an absence of an ion or not!
2. Explain the difference between a confirming test and a distill water bank? What purpose does each serve?
- The difference is that a confirming test is a positive test that confirms that the ion in question is present, while the blank is known not to contain ions.
The purpose the confirming test serves: confirms the presence of an ion
The purpose of blank: has no ions so we can tell if the other substances contain ions.
3. Compare the physical properties of water vs. hydrogen vs. oxygen?
-Water is a liquid the others are gases.
- The reaction when adding a substance to the mixture causes the ion to be so small to the naked eye. So it's impossible to say that there is an absence of an ion or not!
2. Explain the difference between a confirming test and a distill water bank? What purpose does each serve?
- The difference is that a confirming test is a positive test that confirms that the ion in question is present, while the blank is known not to contain ions.
The purpose the confirming test serves: confirms the presence of an ion
The purpose of blank: has no ions so we can tell if the other substances contain ions.
3. Compare the physical properties of water vs. hydrogen vs. oxygen?
-Water is a liquid the others are gases.
Homework #7 Semester 1
25. Qualitative Tests identify the presence or absence of a particular substance in a sample, while, in contrast, Quantitative Tests determine the amount of a specific substance present in a sample.
26. Confirming Tests are positive tests that confirm that the ion in question is present.
27. A. The Reference Solution is known of composition and it's used as a comparison
B. The Distilled-Water Blank is known to not contain any ion of interest.
29. A. I would see if the particles were microscopic, molecular sized, or large and visible.
B. See if the particles were uniform/standard or not.
30. The particles are at the bottom of the bottle so without shaking it, the medicine would not have the same effect as it would if it was shaken.
32.
33. No. It would be too expensive to have absolutely pure, clean, chemical free water.
34. Water (H2O) is composed of two elements (hydrogen and oxygen). At a normal room temperature, water is physically a liquid, while hydrogen and oxygen are both gases.
Monday, June 24, 2013
408 page views! Woohoo! Thanks all you viewers out there! New and exciting things are coming your way! Tomorrow we are starting our second lab! Can we get to 500 views before semester 1 ends? My goal is 1000 by the end of the course!
Tell your friends who love chemistry to view my blog at: http://rioshaneblogspot.blogspot.com/
Check out my new posts!
-Rio
Tell your friends who love chemistry to view my blog at: http://rioshaneblogspot.blogspot.com/
Check out my new posts!
-Rio
Quick Blog Question
How does testing water help us?
Testing water helps us by finding different items in our water we did not know that were in there (and could be something harmful). Some water issues are obvious, but others are invisible so testing water can us find these invisible problems. For instance the possibility of contamination, aging water distribution system, unknown well-water quality, or the type of plumbing in someone's home. Testing water helps us find these problems so that we can have safe and clean water.
Testing water helps us by finding different items in our water we did not know that were in there (and could be something harmful). Some water issues are obvious, but others are invisible so testing water can us find these invisible problems. For instance the possibility of contamination, aging water distribution system, unknown well-water quality, or the type of plumbing in someone's home. Testing water helps us find these problems so that we can have safe and clean water.
Quiz #6 Study Guide
Quiz Study Guide:
1. Electrons
- Negatively charged particles.
2. Protons
- Positively charged particles.
3. Neutrons
- Electrically neutral particles.
4. Ionic Compounds
- Substances composed of positive and negative ions.
5. Cation
- A positively charged ion
6. Anion
- Negatively charged ion.
6. Crystal
- A three-dimensional network where solid sodium ions and negative chloride ions are arranged in.
7. Polyatomic Ion
- An ion consisting of a group of bonded atoms.
8. Two types of copper and iron ions
- Copper: Cu+ and Cu2+
- Iron: Fe3+ and Fe2+
9. Electron Cloud
- The negative space around an electron.
10. Sodium Chloride
- Salt; example of an ionic compound; sodium, chlorine
11. Water
- H20.
12. Memorizing Table (see pg. 40).
- Hydrogen: H+
- Sodium: Na+
- Copper: Cu+, Cu2+
- Silver: Ag+
- Magnesium: Mg2+
- Calcium: Ca2+
- Iron: Fe2+, Fe3+
- Fluoride: F-
- Bromide: Br-
- Hydroxide: OH-
- Oxide: O2-
- (Hydrogen) Carbonate: HCO3-
13. Confirming Test
- A positive test confirms that the ion in question is present
14. Precipitate
- Insoluble material
15. Qualitative Test
- Tests that identify the presence or absence of a particular substance in a sample.
16. Quantitative Test
- Determine the amount of a specific substance present in a sample.
17. Reference Solution
- A solution of known composition used as a comparison.
18. Be able to explain water testing lab
- The steps include:
1. Calcium Ion Test
2. Iron Ion Test
3. Chloride Ion Test
4. Sulfate Ion Test
19. Make your own table
- See pg. 43 in the textbook
20. What is an atom composed of?
- Protons, neutrons, and electrons
21. Ionic compounds: give examples and explain
- Ionic compounds are substances that are composed of positive and negative ions. They have no net electrical charge; they are neutral because the positive and negative electrical charges offset each other.
Example: Table salt (sodium chloride).
22. Potassium and Iodine
1. Electrons
- Negatively charged particles.
2. Protons
- Positively charged particles.
3. Neutrons
- Electrically neutral particles.
4. Ionic Compounds
- Substances composed of positive and negative ions.
5. Cation
- A positively charged ion
6. Anion
- Negatively charged ion.
6. Crystal
- A three-dimensional network where solid sodium ions and negative chloride ions are arranged in.
7. Polyatomic Ion
- An ion consisting of a group of bonded atoms.
8. Two types of copper and iron ions
- Copper: Cu+ and Cu2+
- Iron: Fe3+ and Fe2+
9. Electron Cloud
- The negative space around an electron.
10. Sodium Chloride
- Salt; example of an ionic compound; sodium, chlorine
11. Water
- H20.
12. Memorizing Table (see pg. 40).
- Hydrogen: H+
- Sodium: Na+
- Copper: Cu+, Cu2+
- Silver: Ag+
- Magnesium: Mg2+
- Calcium: Ca2+
- Iron: Fe2+, Fe3+
- Fluoride: F-
- Bromide: Br-
- Hydroxide: OH-
- Oxide: O2-
- (Hydrogen) Carbonate: HCO3-
13. Confirming Test
- A positive test confirms that the ion in question is present
14. Precipitate
- Insoluble material
15. Qualitative Test
- Tests that identify the presence or absence of a particular substance in a sample.
16. Quantitative Test
- Determine the amount of a specific substance present in a sample.
17. Reference Solution
- A solution of known composition used as a comparison.
18. Be able to explain water testing lab
- The steps include:
1. Calcium Ion Test
2. Iron Ion Test
3. Chloride Ion Test
4. Sulfate Ion Test
19. Make your own table
- See pg. 43 in the textbook
20. What is an atom composed of?
- Protons, neutrons, and electrons
21. Ionic compounds: give examples and explain
- Ionic compounds are substances that are composed of positive and negative ions. They have no net electrical charge; they are neutral because the positive and negative electrical charges offset each other.
Example: Table salt (sodium chloride).
22. Potassium and Iodine
Homework Semester 1 #6
Questions 19-24
19. A. Carbon:
- 6 electrons
B. Aluminum:
- 13 protons
C. Lead:
- 82 electrons
D. Chlorine:
- 17 protons
20. A. Not electrically neutral
B. Not electrically neutral
C. Yes electrically neutral
D. Not electrically neutral
21. A. Anion
B. Electrically Neutral Atom
C. Electrically Neutral Atom
D. Cation
E. Cation
22. A. Gaining electrons
B. Neither
C. Neither
D. Losing electrons
E. Losing electrons
23. A. H
B. Na+
C. Cl-
D. Al3+
24. A. Potassium and Iron; K+I-
B. Calcium and Sulfur; Ca2S2
C. Iron and Bromide; Fe3Br-
D. Barium and Hydroxide; Ba2+OH-
E. Ammonium and Phosphate; NH4+PO3-
F. Al3+O2-
B. Aluminum:
- 13 protons
C. Lead:
- 82 electrons
D. Chlorine:
- 17 protons
20. A. Not electrically neutral
B. Not electrically neutral
C. Yes electrically neutral
D. Not electrically neutral
21. A. Anion
B. Electrically Neutral Atom
C. Electrically Neutral Atom
D. Cation
E. Cation
22. A. Gaining electrons
B. Neither
C. Neither
D. Losing electrons
E. Losing electrons
23. A. H
B. Na+
C. Cl-
D. Al3+
24. A. Potassium and Iron; K+I-
B. Calcium and Sulfur; Ca2S2
C. Iron and Bromide; Fe3Br-
D. Barium and Hydroxide; Ba2+OH-
E. Ammonium and Phosphate; NH4+PO3-
F. Al3+O2-
Sunday, June 23, 2013
A7 Questions
#1-7
1. 8,388 Total
Without Gardening: 3,868
2. 1,398 Volume (in Liters)
Without Gardening: 644
3.
4. Range: 1,493
5. Median: 579
6. People tend to have more yards and water them more
7. Mean: 600
Additional Blog Question
What interested you about the first week? What will you remember later?
What interested me in the first week was definitely the foul water lab. I found it really interesting that the charcoal adsorption and filtration was the final and most important step to purifying the foul water since it seemed so dirty. I will also remember this later because we always need to know how to purify water for emergencies.
What interested me in the first week was definitely the foul water lab. I found it really interesting that the charcoal adsorption and filtration was the final and most important step to purifying the foul water since it seemed so dirty. I will also remember this later because we always need to know how to purify water for emergencies.
Saturday, June 22, 2013
Quiz #5 Questions (Semester 1)
1. Interpret Histograms and what they tell us.
- Shows the percent recovery of all lab groups
2. Chemical Symbols
- The letters of the chemical language's alphabet that are understood by scientists throughout the world.
3. Period Table of Elements
- All known elements are organized here; one of the most useful tools in a chemist's world.
4. Subscript
- A number written below the normal line of letters, which indicates how many atoms of the element just to the left of this are in one unit of the substance.
5. Chemical Equations
- Chemicals sentences that summarize the details of a particular chemical reaction.
6. Chemical Reactions
- Entail the breaking and forming of chemical bonds, causing atoms to become rearranged into new substances.
7. Reactants
- The original (starting) substances in a chemical reaction (written to the left of the arrow)
8. Products
- The new substance or substances formed from from the rearrangement of the reactant atoms.
9. Balanced Equations
- The total number of each type of atoms is the same for both reactants and products.
10. Diatomic Molecules
- They exist as two bonded atoms of the same element.
- Shows the percent recovery of all lab groups
2. Chemical Symbols
- The letters of the chemical language's alphabet that are understood by scientists throughout the world.
3. Period Table of Elements
- All known elements are organized here; one of the most useful tools in a chemist's world.
4. Subscript
- A number written below the normal line of letters, which indicates how many atoms of the element just to the left of this are in one unit of the substance.
5. Chemical Equations
- Chemicals sentences that summarize the details of a particular chemical reaction.
6. Chemical Reactions
- Entail the breaking and forming of chemical bonds, causing atoms to become rearranged into new substances.
7. Reactants
- The original (starting) substances in a chemical reaction (written to the left of the arrow)
8. Products
- The new substance or substances formed from from the rearrangement of the reactant atoms.
9. Balanced Equations
- The total number of each type of atoms is the same for both reactants and products.
10. Diatomic Molecules
- They exist as two bonded atoms of the same element.
Friday, June 21, 2013
Homework Day #5 Semester 1
ISBS Questions #13-18
13. See drawing
14. Elements: i, ii, vi
Compounds: iii, iv, v
15. Represents a different chemical substance and a chemical symbol that represents each element present.
16. A. Elements: H, P, O
Atoms: 3, 1, 4
B. Elements: Na, O, H
Atom: 1, 1, 1
C. Elements: S, O
Atoms: 1, 2
17. See drawing.
18. See drawing.
13. See drawing
14. Elements: i, ii, vi
Compounds: iii, iv, v
15. Represents a different chemical substance and a chemical symbol that represents each element present.
16. A. Elements: H, P, O
Atoms: 3, 1, 4
B. Elements: Na, O, H
Atom: 1, 1, 1
C. Elements: S, O
Atoms: 1, 2
17. See drawing.
18. See drawing.
Thursday, June 20, 2013
Semester 1: Test #1 Review.
Test #1: Review
Part 1: In Class Review
Chlorine: Added to all tap water to kill bacteria. It's reactive and kills the bacteria right away.
Hydrologic Cycle: Water gets evaporated to vapor then goes to the the sky and gets precipitated then down back into the ocean. A cycle is a closed system so no water is created or destroyed.
Catalyst: A substance that increases the rate of a chemical reaction without itself undergoing any permanent chemical change. You add a catalyst to a chemical reaction. It speeds up a chemical reaction.
Law of Conservation of Matter: No matter is created or destroyed, it's all conserved.
Aqueous Solutions: A water-based solution.
Fe: Iron
O: Oxygen
Al: Aluminum
N: Nitrogen
Au: Gold
Na: Sodium
Ag: Silver.
Part 2: Test Question:
1. Review indirect vs. direct water use?
- Hidden vs. obvious uses of water.
2. Review what two things combined make homogeneous vs. heterogeneous mixtures?
- Homogeneous: Substances and solutions.
- Heterogeneous: Colloids and suspensions.
3. Review the Celsius temp scale?
- Boiling/100 degrees C and Freeze/O degrees C
- Boiling/-212 degrees F and Freeze/32 degrees F.
4. Smallest unit of an element?
- An atom.
5. Are all solutions homogeneous?
- Yes!
6. The dissolved substance in a solution is the (solvent? solute?)
- Solute.
7. A solution is one type of (element? compound? mixture?)
- Mixture.
8. Explain differences and give examples between solution, colloid, and suspension.
- Suspensions and colloids are both heterogeneous mixtures while solutions are homogeneous.
9. Which is a compound? CO or Co?
- CO.
10. Fluoride is added to drinking water for what purpose?
- It's for anti cavity purposes.
11. Chlorine is added to drinking water for what purpose?
- To kill bacteria.
12. Why is distillation not used to purify most tap water?
- Too expensive.
13. Explain the use of gray water?
- The relatively clean waste water from baths, sinks, washing machines, etc so you get to use the water twice.
14. Define the hydrologic cycle?
- Water gets evaporated to vapor then goes to the the sky and gets precipitated then down back into the ocean. A cycle is a closed system so no water is created or destroyed.
15. Particles with the same charge put close together do what?
- They repel each other.
16. pH scale measures what?
- Measures hydrogen concentration
17. Define portable water?
- Drinking water or potable water is water safe enough to be consumed by humans or used with low risk of immediate or long term harm.
18. Draw a mixture of one element and one compound.
- See drawing.
19. A molecule that is positively charged on one end and negatively charged on the other is ____
- Polar
20. 100 gm of 25% sugar solution contains how much water and how much sugar?
- 25% sugar and 75% water.
21. An atom is the smallest particle of ______.
- Element.
22. Define and give a definition of a physical property of a substance.
- Physical property: properties that can be observed and measured without changing the chemical makeup of the substance.
- Substance: homogeneous, definite composition and not physically separable.
23. Tyndall effect proves what?
- Shows particles in suspension.
24. After filtration, if there is no Tyndall effect?
- The particles are not in suspension.
25. Two elements bonded in a definite proportion: _____
- FeLi
26. 2 L bottle can pour how many 250 mL servings?
- 250000.
27. How is the earth's water distributed, from most to least?
Oceans, glaciers, water vapor, rivers.
28. Why do ice cubes float?
- They have less density.
29. Why don't we drink absolutely fresh water?
- Too expensive.
30. Subscripts and what they mean?
- The number in a compound that let us know how many atoms of an element are there.
31. What are the three states of water?
- Solid, liquid, gas.
32. What is the freezing and boiling points of water in centigrade (Celsius) and in Fahrenheit?
- Celsius: In boiling, 100 degrees and in freezing point, 0 degrees
- Fahrenheit: -32: freezing and -212: boiling.
33. What is the density of water? What are the units?
- 1 gram per mL and 1 cm by cubic centimeter OR 1.00 gram = 1 mL
34. What is the purpose of the foul water lab? How does it have significance in the real world?
- The purpose of the foul water lab was to purify dirty water. It's significance in the real world shows that we can purify our own water.
35. Describe the Tyndall effect.
- Scattering of light; small particles scatter the light (colloids, suspensions)
36. What is a solution?
- Homogeneous, often molecular sized particles that can pass light.
37. Solvent?
- The dissolving agent.
38. Solute?
- The dissolving substance.
39. Use the chart on pg. 30 to explain the difference between colloids and solutions and suspensions.
- Colloids and suspensions are heterogeneous while solutions are homogeneous.
Define the following terms (and give examples).
40. Physical Property
- Properties that can be measured and observed without changing the chemical makeup of the substance.
41. Matter
- Anything with space and mass.
42. Density
- The mass of material within a given volume.
43. Freezing point
- Type of physical property.
44. Aqueous solution
- Water-based solution
45. Surface tension
- The tension of a surface in which particles attract.
46. Melting point
- Physical property
47. Boiling point
- Physical property
48. Suspension
- Blocks light, visible particles. Heterogeneous.
49. Mixture
- Homogeneous and heterogenous; combining
50. Heterogeneous Mixture
- Different, not uniform.
51. Tyndall effect
- Scattering of light.
52. Colloid
- Exhibit Tyndall effect
53. Homogeneous Mixture
- Same, uniform
54. Solution
- Homogenous, particles that can pass light.
55. Solvent
- Dissolving agent.
Part 3: More terms to know
Quantity: Unit: Abbreviation
1. Mass: Kilogram: kg
2. Length: meter: m
3. Time: second: s
4. Temperature: kelvin: K
Prefix: Abbreviation: Meaning
1. kilo: k: 10'3 (ten to the 3rd)
2. deci: d: 10'-1 (ten to the negative 1st)
3. centi: c: 10'-2 (ten to the negative 2nd)
4. milli: m: 10'-3 (ten to the negative 3rd)
5. micro: u: 10'-6 (ten to the negative 6th)
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