1. Chemistry SOL Review Day 2

2. UNIT 6 – Ionic Bonding
The electrons in the outermost level or shell are called the ________________ electrons.
 Valence
Atoms want to be stable, which means they try to achieve a ____________________ configuration.
 Noble Gas
To become an ion, atoms will ______________ or ________________ electrons.
Gain or lose

3. UNIT 6 – Ionic Bonding What kind of ion does Calcium become? 2+
A bromine ion (Br-) has ________ electrons and _______ protons.
 36, 35
A magnesium ion (Mg2+) has _________ electrons and _______ protons.
10, 12

4. UNIT 6 – Ionic Bonding A cation is a _________ charged ion. Positively
An anion is a _____ charged ion.
 Negatively
Ionic bonds form between ___ &_____.
Positive & negative ions
Metals & Nonmetals

5. UNIT 6 – Ionic Bonding
Ionic compounds have ________ melting points because of the strong forces within.
High
An alloy is a mixture of two __________.
Metals

6. UNIT 6 – Ionic Bonding Name the following ionic compounds. KBr K2O
MgBr2
Cu(OH)2
Ca3(PO4)2

7. UNIT 6 – Ionic Bonding
Write formulas for the following ionic compounds.
Copper (I) oxygen
Aluminum oxide
Lead (IV) sulfide
Lead (IV) nitride
Lithium chloride

8. 2009 SOL Question
How many electrons does the iron ion have when it forms the ionic compound FeCl3?
F 20
G 23.
H 26
J 29

9. UNIT 7 – Covalent Bonding
When two nonmetals join together, they form a covalent bond by __ their electrons.
Sharing
Most atoms that form covalent bonds connect so each atom has _____ valence electrons. 8

10. UNIT 7 – Covalent Bonding
Name the 7 diatomic elements
Name the following molecular compounds.
N2O
CO2
C2H6
H2S
N2O4

11. UNIT 7 – Covalent Bonding
Write the chemical formula for each of the following molecular compounds.
Carbon monoxide
Dihydrogen monoxide
Phosphorus trichloride
Carbon tetrahydride
Dicarbon tetrahydride

12. UNIT 7 – Covalent Bonding
Draw the Lewis structure or structural formula of each of the following and determine its shape.
SiCl4
SCl2
PF3
AsF5
BF3

13. UNIT 7 – Covalent Bonding
If there is a LARGE difference in electronegativity, it will result in a ____________ bond.
Ionic
A medium difference in electronegativity will result in a _________ covalent bond.
Polar
A very small difference will result in a ____ covalent bond.
Nonpolar

14. UNIT 8 – Chemical Reactions
The chemicals used to start a chemical reaction are called the _____
Reactants
The chemicals that come out of a reaction are the _____
Products
If something is written above the arrow, it is a _____
Catalyst

15. UNIT 8 – Chemical Reactions
Balance the following reactions.
a. CuCl H2S  CuS HCl
B. Fe + O2  Fe2O3
c. P + O2  P4O10
d. Na + H2O  H2 + NaOH
e. FeCl3 + CaOH  Fe(OH)3 + CaCl

16. UNIT 8 – Chemical Reactions
Classify the following reactions (synthesis, decomp, SR, DR, or combustion)
4Fe + 3O2  2Fe2O3
2C6H O2  14 H2O + 12 CO2
2AlCl3  2Al Cl2
Zn + H2SO4  Zn SO4 + H2
AgNO3 + NaCl  AgCl + NaNO3

17. UNIT 9 – Molar Conversions
The _____ is the lowest whole number ratio of elements in a compound.
Empirical formula
The __________ formula is the actual ratio of elements in a compound.
Molecular formula

18. UNIT 9 – Molar Conversions
What is the empirical formula of C6H12O6?
 CH2O
What is the empirical formula of C3H6?
 CH2
A compound has an empirical formula of ClCH2 and a molar mass of g/mol. What is its molecular formula?
Cl3C3H6

19. UNIT 9 – Molar Conversions
Calculate the percent composition of sodium in sodium chloride (NaCl).
23/( ) = 39%
1 mole = how many particles?
6.022 x 1023
How many atoms of oxygen are in a 17.3 g sample?
6.51 x 1023