Name: ____________________________
1st attempt score: _____/41
2nd attempt score: _____/41
CPE pretest (Ch. 5, 6.3): Chemical bonds, compounds, reactions
1. __J__ another name for a charge on an ion
A. anion
2. __G__ when two or more atoms gain/lose electrons when
B. cation
forming a compound they form charged particles
C. charge
that are attracted to each other. Happens
D. covalent bond
between metals and nonmetals.
E. coefficient
3. __F__ a structure that has two atoms per molecule.
F. diatomic molecule
Some examples are: N2, O2, F2, Cl2, Br2, I2, and H2.
J. oxidation number
4. __L__ an ion that has more than one atom to it, but it acts
G. ionic bond
like only one atom, e.g. OH– , SO42-, NH4+
H. metallic bond
5. __M__ a number written small and after an element to show
I. nonpolar bond
how much of that element there is in a compound
J. oxidation number
6. __A__ name for any ion with a negative charge
K. polar bond
7. __I__ a covalent bond in which the electrons
L. polyatomic ion
are shared equally
M. subscript
8. __H__ a bond between atoms of the same metal element, not between atoms of different elements.
It allows for many special properties.
9. __C__ will be positive if the atom loses electrons or negative if it gains electrons
10. __E__ a large number written before a compound to show how much of that compound is in
a chemical reaction
11. __D__ bond in which atoms share electrons, between two nonmetals.
12. __B__ name for any ion that has lost electrons and has positive charge
13. __K__ a covalent bond in which the electrons are not shared equally; results in partial charges
on the molecule
Determine the total number of atoms of each element in the following compounds.
14. C2H4
C = ___2____
H = ____4___
15. H3PO4
H = ___3____ P = ___1____
O = ____4___
16. Ni(OH)2
Ni = ___1____ O = ___2____ H = ___2____
17. Metals tend to ___lose___ electrons and form _____________positive ions________________ ions.
18. Nonmetals tend to ______gain__________ electrons, form _______negative ions_____________ ions
and can be found on the ____right____ hand side of the periodic table.
19.–20. Here is a periodic table. Draw the Lewis diagram and label the charge (oxidation #) of each group.
Skip groups 3–12 (transition elements).
+1
+2
+3 +-4 –3
–2
–1
0
X∙
∙X∙
∙ Ẋ ∙
∙
∙ X∙
∙
∙
:X∙
∙
∙
∙∙
∙∙
:X : :X : :X :
∙
∙
∙∙
21. _______ionic_______ bonds form between metals and nonmetals when electrons are
____________________transfered (lost by a metal and gained by a nonmetal)______________________.
22. _________covalent________________ bonds form between two nonmetals when electrons are
_________________shared_____________________________________________.
Identify the following as ionic or covalent bonds.
23. _________covalent_____________ CO2
24. _________ionic and covalent_____________ (NH4)2O
25. _________ionic_____________ FeI3
Determine the charge on each metal ion in bold.
26. ____+1____ Ag2O
27. ____+3_____ Fe2O3
28. ____+2_____ CuSO4
Use Lewis diagrams to show the bonding between the following atoms. Write the resulting compound.
Clearly indicate whether electrons are shared, gained or lost.
29. Na + S
30. C + F
∙∙
Na ∙ →∙ S ∙←∙ Na
∙∙
Na 2 S
∙∙
:F:
∙
∙∙
∙
∙∙
: F∙ ∙ C ∙ ∙ F:
∙∙
∙
∙∙
∙
:F:
∙∙
CF 4
∙∙
:F:
∙
∙∙
∙
∙∙
: F∙ ∙ C ∙ ∙ F:
or
∙∙
∙
∙∙
∙
:F:
∙∙
CF 4
Write the name of the compound for each example given.
31. _____lithium nitrate______________________ LiNO3
32. _____calcium chloride______________________ CaCl2
33. _____sulfur dibromide______________________ SBr2
Write the formula for each compound given.
34. ____MgI2________ magnesium iodide
35. ____P2O3________ diphosphorus trioxide
36. ____SrSO4________ strontium sulfate
Balance the following chemical equations.
37.
__2___ Fe + __3___ Cl2 → __2___ FeCl3
38.
__3___ H2 + _____ N2 → __2___ NH3
39.
_____ CaCl2 + __2___ AgNO3 → __2___ AgCl + _____ Ca(NO3)2
Write and balance the following chemical equations.
40. Chlorine gas reacts with potassium bromide to form potassium chloride and bromine.
Cl2 +
KBr →
KCl +
Br2 (unbalanced)
Cl2 + 2 KBr → 2 KCl +
Br2 (balanced)
41. Calcium oxide reacts with sulfur dioxide to form calcium sulfite.
CaO +
SO2 →
CaSO3
(already balanced)