Example of Chemical Reactions Lab

Make sure to complete all the questions to the lab.

Examples of Chemical Reactions

1. Balance the following chemical reactions. Make sure to use the correct chemical formula and the state for each substance.

a. Solid magnesium reacts with aqueous hydrochloric acid to produce aqueous magnesium chloride and hydrogen gas.

b. Aqueous sodium chloride reacts with aqueous silver (i) nitrate to produce solid silver (i) chloride and aqueous sodium nitrate.

c. Solid magnesium burns in the air to form solid magnesium oxide.

2. Observations  (make sure they are complete and descriptive):

Part 1: __________________________________

Part 2: __________________________________

Part 3: __________________________________

Part 4: __________________________________

3. For each of the reactions, what observations did you make that indicated a chemical reaction was taking place.

4. What are some clues that accompany chemical changes?

5. When balancing chemical equations what is the number you can change and what does it represent? What number can you not change and what does it represent?

Homework for 11/17

1) Read chpt 6
2) pg. 176  ex 6.1, pg. 177 ex 6.2, pg. 184 ex 6.4, #2, 4-5
2) HW drop in M, W & F next week
3) Have g-mail account by Wednesday
4) All Chpt 7 HW due Monday!
5) Composition books due

Homework for 11/13

1) pg. 232 #1-4, pg. 234 #9-20
2) HW drop in Friday
3) Get a g-mail account, if you have one make sure to know your password and user name
4) Chapter 7 & 12 Test Friday!
5) All late homework for Chapter 7--last chance to turn in is Monday 12/17

Homework for 11/12

1) pg. 223 exercise 7.1 a-c, pg. 223 #1, 3-4, pg. 232 exercise 7.4 a-c
2) HW drop in Friday
3) Tutoring after school Wednesday!
4) Chapter 7 & 12 Test Friday!

Study Guide for Test 11/14

Chapter 12

Answers to Chpt 12 practice pg. 439
1. C
2. D
3. B
4. C
5. D
6. A
7. B
8. C
9. a. tetrahedral   b. trigonal planar   c. trigonal pyramid

What to study for Chpt 12
--types of bonds: what is difference between ionic, covalent an polar covalent
--what are the properties of an ionic bond
--understand what is electronegativity and what elements have the highest/lowest electronegativity
--what is a dipole moment in a molecule and be able to tell what is the positive and negative side of the bond
--know what are the charges that elements in groups 1-8 make when they form an ion
--know what will be the formula when two elements form a compound by their ionic charges
--know how to make Lewis structures for covalent compounds
--know that all atoms (except hydrogen and helium) are looking for eight electrons due to the octet rule
--know how to recognize a lone pair and a bonded pair of electrons in a Lewis structure
--know what VSEPR model or shape that the molecule will take based on its Lewis structure

Chapter 7:

Practice test pg. 237
1. D
2. B
3. C
4. D
5. A
6. B
7. C

9. Mg (s) + 2H₂O (l)   arrow         H₂ (g) + Mg(OH)₂ (aq)

10. Pb(NO₃)₂ (aq) + 2NaI (aq) arrow  PbI₂ (s) + 2NaNO₃ (aq)

11. C₃H₈ (g) + 5O₂  arrow   3CO₂ (g) + 4H₂O (g)

12. 2Ca(s) + O₂ (g)   arrow   2CaO (s)

 
--know what are the signs of a chemical reaction
--what makes a reaction chemical as opposed to physical
--how to make formulas for a chemical equation
     --keep in mind roman numerals for transition metals
     --remember that gases and halogen elements are always diatomic and have two atoms