Practice Test Chemical Bonds and Compounds
1. Use electronegativity values to determine if the bonds formed between
each of the following atoms would be ionic, covalent, or polar covalent
Ni & Cl _____
Br & S _____
F & P _____
S & Ba _____
O & P _____
Fe & F _____
I & C _____
Mg & O _____
2.
15. What is Avagadro’s Number?
16. What is the formula weight of
Carbon
SiO2
Mg(NO3)2
Na2S
17. What is the mass of
3 moles of Calcium
7 moles of CO2
5.44  1025 atoms of Silver (Ag)
3.68  1022 molecules of NCl3
18.
How many moles are there in
148g of gold
178g of CaCl2
67g of (NH4)2S
19. How many Atoms of Fluorine are there in 4 moles of CF4? _______________
How many Moles of Oxygen are there in 4 moles of Al(NO3)3? _______________
How many atoms of Oxygen are there in 4 moles of Al(NO3)3? _______________
How many grams of Oxygen are there in 245g of CO2? __________________
20. For each of the following molecules, determine if the bonds are covalent or polar covalent.
Next, determine if it is a polar molecule, write “yes” if it is, and “no” if it is not.
Compound
SiO2
NF3
SO2
molecular shape
(linear)
(trigonal pyramidal)
(bent)
bond type
polar molecule (Y/N)
_______________
_______________
_______________
_______________
_______________
_______________
CH4
(tetrahedral)
_______________
_______________
SO3
(trigonal planar)
_______________
_______________
21.
Air is a mixture of roughly 80% N2, and 20% O2 which element is the solvent?
22.
Which of the following compounds would you expect to be soluble in SBr 2 (a bent molecule)?
(hint: look at the electronegativity values) H2O
SeBr2
SF2
NF3
23.
How many moles of H2SO4 are there in 400 ml of a 6 M solution?
24.
How many grams of BaCl2 are there in 250 ml of a 7.4 M solution?
25.
How many Chloride ions are there in 150 ml of a 0.06M solution of AlCl 3?
26.
How many ml of 6.0 M NaCl solution would you need in order to prepare
125 ml of 0.5 M NaCl solution?
(look at the graph above to answer questions 27 – 29)
27. How many grams of Calcium Chloride can be dissolved in 100 g of water at 20C?
28. How hot would the water have to be in order to get 70g of K 2Cr2O7 to dissolve in 100g of water?
29. If a 60g crystal of Pb(NO3)2 was put in 100g of water at 20C, how much of the crystal would
be left after it dissolved?
Answers to Practice Test Chemical Bonds and Compounds
1. an element has only one kind of atom, a compound is made of two or more different kinds of atoms
2. an ionic compound is formed between a metal and a non-metal and involves electrons leaving the metal
atom and joining the non-metal atom. A covalent compound involves two non-metals that share electrons.
3. In a solution the largest particle is an atom, molecule, or ion
4. metal
5. ionic compound 6. noble gas
7. covalent bond 8. ionic bond 9. O2 and Ca
10.
Al & O ionic
F & Ne none
Ni & Cr no
N & I covalent
C & Cl covalent
Pb & S inoic
Ar & S none
Na & P ionic
11. sodium oxide
ammonium sulfide
12. Cu3PO4
13.
dinitrogen hexaoxide
silicon dioxide
P2O5
MgF2
Ni & Cl polar covalent
O & P polar covalent
lead(II)hydroxide
iron (II) sulfate
Cr(ClO2)6
Fe2O3
Br & S covalent
Fe & F ionic
NBr3
F & P ionic
I & C covalent
S & Ba polar covalent
Mg & O ionic
14.
15. 6.02  1023
16. C: 12.011
SiO2: 60.065 Mg(NO3)2 :148.24 Na2S: 78.044
17. 120.234 307.937 9747.558 7.357
18. gold: 0.75 moles
CaCl2: 1.60 moles (NH4)2S: 0.98 moles
19. CF4: 9.63  1024
Al(NO3)3: 36 moles
Al(NO3)3: 2.17  1025 atoms
CO2: 178.13 g
20.
SiO2 polar, no
CH4 covalent, no
NF3 polar, yes
SO3 Polar, no
SO2 polar, yes
21. N2 because there is more of it
22. SeBr2 because it is non-polar and so is SBr2
23. 2.4 moles
24. 385.23 g
25. 1.6  1022
26. 10.4 ml
27.  75g
28.  90C
29 5g