Honors CHEMISTRY (p. 5&6)
Writing and Naming Compounds Review
Name: ____________________________
____ period
1.
What is a cation and how is it formed?
(+) ion – atom loses electrons
2.
What is an anion and how is it formed?
(-) ion – atom gains electrons
3.
What is an ionic bond and how is it formed?
Formed when atoms transfer electrons
Form from cations and anions which form an electrostatic attraction bond
What properties do ionic compounds have?
High melting and boiling points
Form electrolytes in H2O – conduct electricity
Form crystals
most are salts
4.
5.
6.
Write the formulas for the following ionic compounds:
a.
sodium sulfate
Na2SO4
b.
barium chloride
BaCl2
c.
potassium nitrate
KNO3
d.
copper(II) sulfide
CuS
e.
iron(III) acetate
Fe(C2H3O2)3
f.
magnesium nitride
Mg3N2
Write the names for the following ionic compounds:
a.
Na3PO4
sodium phosphate
b.
Ag2CO3
silver carbonate
c.
MgF2
magnesium fluoride
d.
(NH4)3P
ammonium phosphide
e.
CuBr2
copper (II) bromide
f.
FeSO4
iron (II) sulfate
7.
What is a metallic bond?
Bond between atoms of metal – results from shared electrons – “sea of delocalized electrons”
8.
What properties do metallic bonds give to metals?
Malleable, ductile, good conductors, luster, high melting and boiling points
9.
What is a covalent bond?
Chemical bond in which 2 atoms share a pair of electrons (nonmetals)
10.
What properties do covalent compounds have?
Brittle, solid, liquid or gas at room temp, dull color, poor conductors, low melting and boiling points
11.
What are the seven diatomic elements? What kind of bonds do they have?
Br2 O2 F2 I2 N2 Cl2 H2 (BO FINCH)
Covalent
12.
What is a single bond? How strong is it compared to double and triple bonds?
Covalent bond with 1 pair of electrons (2 electrons) – weak compared to double and triple
13.
What is a double bond? How strong is it compared to single and triple bonds?
Covalent bond with 2 pairs of electrons (4 electrons) – stronger than single, weaker than triple bond
14.
What is a triple bond? How strong is it compared to single and double bonds?
Covalent bond with 3 pairs of electrons (6 electrons) – stronger than single and double bonds
15.
Give the prefixes used in naming covalent compounds and tell how many atoms they represent.
Mono-1, di-2, tri-3, tetra-4, penta-5, hexa-6, hepta-7, octa-8, nona-9, deca-10
16.
Name the following covalent compounds:
17.
a.
CO2
carbon dioxide
b.
P2O5
diphosphorus pentoxide
c.
AsCl3
arsenic trichloride
d.
H2O
dihydrogen monoxide
e.
N2H4
dinitrogen tetrahydride
f.
SO3
sulfur trioxide
Write the formulas for the following covalent compounds:
a.
nitrogen monoxide
NO
b.
dinitrogen pentoxide
N2O5
c.
sulfur hexafluoride
SF6
d.
decaphosphorus tetroxide
P10O4
e.
dihydrogen dioxide
H2O2
f.
phosphorus trichloride
PCl3
18.
What are the rules for naming acids?
Binary – hydro + name with –ic acid
Ternary – root of name of anion, change –ate ending to –ic and –ite ending to –ous + acid
19.
Name the following acids:
20.
21.
a.
HBr
hydrobromic acid
b.
HNO2
nitrous acid
b.
HCl
hydrochloric acid
d.
H2CO3
carbonic acid
e.
H2SO4
sulfuric acid
Write the formulas for the following acids:
a.
hydrofluoric acid
HF
b.
phosphoric acid
H3PO4
c.
nitric acid
HNO3
d.
acetic acid
HC2H3O2
e.
chlorous acid
HClO2
Draw Lewis structures for the following compounds and tell whether they are ionic, polar covalent,
or nonpolar covalent compounds:
a.
SO3
polarity polar
b.
H2O
polarity polar
c.
C2H4
polarity nonpolar
d.
CO2
polarity nonpolar
22.
What is electronegativity?
Measure of an atom’s attraction for a pair of electrons in a bond
23.
How can you use electronegativities to determine the type of bond formed between two elements?
1.7-4.0
ionic
0.3-1.7
polar covalent
0.0-0.3
nonpolar covalent
Determine the bond types between the following elements:
24.
a.
H and O
polar covalent
b.
Na and I
polar covalent
c.
Mg and N
ionic
d.
Sr and F
ionic
e.
P and S
polar covalent
f.
C and I
nonpolar covalent
25. Molecular Geometries (these examples are in your notes)
compound
CO2
total
areas
of e2
shared
pairs
of e2
lone
pairs
of e0
CH4
4
4
0
Lewis Structure
Name of Molecular
Shape
Polarity
linear
nonpolar
tetrahedral
nonpolar
26. Predicting Molecular Shapes
Draw each molecule and predict the shape each molecule will form.
IBr5
CCl4
Shape: trigonal bipyramidal (polar)
Shape: tetrahedral (nonpolar)
PCl3
H2 S
Shape: trigonal pyramidal (polar)
C2H2
Shape: linear (nonpolar)
Shape: linear (nonpolar)
Shape: trigonal pyramidal (polar)
SO3