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Game
H
FAP)
Directions: Atoms are lonely hearts that are constantly in search of partners to bring stability to their lives. Yourjob is
to play matchmaker and make each atom stable by determining how many valence electrons each element needs and
finding a partner that will complete the valence energy level.
Part 1: Let's meet our first bachelor, Mr. Sodium. Mr. Sodium is very lustrous but has an explosive personality when he
gets near water or oxygen. He is quite a lonely metal that, like all metals, is looking to lose a few electrons! Since he is
highly reactive... so be careful with who you pick to be his date !
ln the circle to the right, create an Bohr model of Mr. Sodium.
Sodium-24
p
no
e'
Let's meet our eligible bachelorettes:
Ms. Lithium is a highly reactive
Ms. Calcium is a reactive
Ms. Fluorine is a nonmetal
metal looking to lose electrons.
metal looking to lose electrons
looklng to gain electrons.
Calcium-40
Lithium-7
Fluorine -18
p
p
p'-
no
no
no
e'
e-
e
Mr. Sodium should date
beca use
Draw the Lewis dot structure for the bonded compound in the space below.
Let's meet our next available bachelorette, Ms. Oxygen. Ms. Oxygen is a lonely non-metal who, like all
non-metals, is looking to gain a few electrons! While she is needed by many living things, she is having a
hard time finding love.
ln the circle the right, create a Bohr model of Ms. Oxygen.
Oxygen-16
p
no
e'
Let's meet our eligible bachelors:
Mr. Sulfur is a highly reactive
Mr. Magnesium
nonmetal looking to gain an electron
metal looking to lose electrons
Sulfur-32
Magnesium-24
p-
p'
p
n'
no
no
e-
e'
e'
Ms. Oxygen should date
is a
reactive
Mr. Phosphorus a nonmetal
looking to gain electrons.
because
Draw the Lewis dot structure for the bonded compound in the space below.
Phosphorus-32
Bonding Basics
Section
A:
chl9a
Complete the chart using a periodic table to help you.
Element
Total # of
Electrons
Atomic
Symbol
# of Valence
Electrons
# of Electrons
Needed to
Gain or Lose
(to
v
Oxidation
Number
Fill Outer Shell)
Chlorine
Potassium
Magnesium
Fluorine
Aluminum
Sodium
Nitrogen
Oxygen
Hydrogen
Carbon
Iodine
Answer these questions:
.
.
An atom that gains one or more electrons will have
a
charge.
An atom that loses one or more electrons will have
a
charge.
.
An atom that gains or loses one or more electrons is called an
'
A positive ion is called
a
and a negative ion is called an
Section B: Ionic Bonds
What is an ionic bond?
.
'
.
to another to form the bond.
Atorns will transfer one or more
Each atom is left with a
outer shell.
An ionic bond forms between a
ion with a negative charge.
Sodium + Chlorine
-
Potassium
Calcium
* Iodine
* Chlorine
AUrninu'rn + Or13en
ion with a positive charge and
a
Magnesium + Iodine
Sodium + Orygen
Aluminum
*
Chlorine
Mag:situn + Ni*o3cn
'
Nome
Trodilionol Chemistry
lonic Formulos Worksheel
Dole
Period
Direclions: Use the criss-cross method lo wriie the formulos for ionic compounds mode of the
cofions (lisied in verticol) ond onions (listed ocross ihe top).
Br-
Co2*
No*
Al3t
Cs*
Cu2*
Mg2*
Zn2*
Fe3*
Crs*
NHat
H+
s2-
P3-
oH-
NOs-
SOa2-
CO:2-
POn3-
Writing formulas and Naming - Binary ionic compounds
Write the ions formed
1.
Sodium chloride
2.
Magnesium fluoride
3.
Calcium bromide
4.
Boron phosphide
5.
Magnesium oxide
6.
Aluminum sulfide
7.
Potassium nitride
8.
Beryllium iodide
9.
Rubidium nitride
10, Cesium carbide
Write the name of the compound
I 1. CaS
12. Balz
13. K2O
15. SrS
17. MgO
18. Na:N
19. BeCl"
20.GarS,
Write the formula
Writing formulas and naming - Ternary ionic compounds
Write the ions formed
l.
Sodium chlorate
2.
Magnesium fluorite
3.
Calcium bromate
4.
Ammonium phosphide
5.
Magnesium chromate
6.
Aluminum sulfite
7.
Potassium nitrate
8.
Beryllium iodate
9.
Cesium acetate
10. Lithium hydroxide
Write the name of the compound
I 1. CaCOr
12. K2C2O
14. Ba(IO:)z
15. SrdPO,),
'15.
NaMnO
17. NaOH
18. NFI4NO3
19. MgSO:
20. Ca(HSO+)z
Write the formula
Writing formulas and naming - Binary ionic compounds with
group 3-12, or 14 metals
Write the ions formed
1.
Coper (II) chloride
2.
Tin (IV) fluoride
3.
Lead (IV) bromide
4.
Imn (III) phosphide
5.
Tin (II) oxide
6.
Iron (III) sulfide
7.
Silver nitride
8.
Zinc iodide
9.
Cadmium bromide
10. Vanadium (VI) oxide
Write the name of the compound
1
1. FeS
13. Cu2O
14. PbF,
15.
16. FeCl:
17. CrO
19. SnBr
20. Ag3N
Write the formula
Writing formulas and naming - Ternary ionic compounds with
group 3-12, or 14 metals
Write the ions
L
Coper
2.
Tin (IV) bromate
3.
Silver phosphate
4.
Cadmium chromate
5.
Copper
6.
Cobalt (II) nitrate
7.
Lead
8.
Tin (II) nitrate
9.
Lead (IV) sulfate
formed
(II) chlorate
(II) sulfite
(IV) iodate
10. Manganese (trI) bicarbonate
Write the name of the compound
1
'
1. FeCrOr
12. cd(to3)z
13. CuzCzOo
14. ZnCO3
15. Pb3(PO4)'
16. MndSO)3
17. Cu(NO2)z
18. Snr(POs)"
19. CuOH
20. CrAsOr
Write the formula
Writing formulas and naming - Acids
Write the ions
21
formed
. Hydrocyanic acid
22. Dichromic acid
23. Hydrobromic acid
24. Nitrous acid
25. Sulfuric acid
26. Acetic acid
27, Carbonic acid
28. Sulfurous acid
29. Phosphoric acid
30. Hydroselenic acid
Write the name of the compound
31. H2SiO3 (aq)
32. HF (aq)
33. HrS
34. H3PO3 (aq)
3s. HClo (aq)
36. H:P (aq)
37. HMnOr (aq)
38. HCI (g)
39. HCIOz (aq)
40.HrCrOn
Write the formula
Mixed NOMENCLATURE Practice
Ionic Compounds & Acids
NAME THE FOLLOWING COMPOUNDS:
1.
BaSO:
11.
AgNO3
2.
(N}I4)3PO4
12.
FezOt
3.
MgSOr
13. HCIO
4.
Ca(OH),
14.
HF
5.
H3PO4
15.
HrCrO4
6.
NazCru
16.
NaHCO:
7.
MgO
17.
CuClz
8.
Cu(NO3)2
'18. HNO,
9.
HI
19.
SnOz
20.
BaCrOr
Or
10; MnO
WRITE FORMULAS FOR T}IE FOLLOWING COMPOUNDS:
.
mercury(Il) iodide
21 . hydrobromic acid
31
22. chromium(Ill) carbonate
32.
sulfurous acid
23. magnesium sulfide
33.
lead(Il) nitrate
24. lithium hydride
34.
sodium oxalate
25. ammonium hydroxide
35. perchloric acid
26. calcium chloride
36. chlorous acid
27. hydroselenic acid
37. carbonic acid
28. iron(Il) nitride
38. sodium chlorate
29. aluminum hydroxide
20
30. tin(II) fluoride
40. potassium perchlorate
nickel nitrate