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Name: 
 

Chpater 10,11 and 12



Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

1. 

Each inner energy level of an atom has maximum numbers of _____ it can hold.
a.
electrons
c.
quarks
b.
neutrons
d.
protons
 

2. 

Dot diagrams are used to represent _____.
a.
atomic numbers
b.
atomic mass
c.
isotopes
d.
outer electrons
e.
the structure of the nucleus
 

3. 

A chemical symbol represents the _____ of an element.
a.
name
b.
reaction
c.
group
d.
structure
e.
type
 

4. 

Horizontal rows of the periodic table are called _____.
a.
clusters
b.
families
c.
groups
d.
periods
e.
quarks
 

5. 

Atoms of the same element with different numbers of neutrons are called _____.
a.
isotopes
b.
metals
c.
metalloids
d.
radioactive
e.
transition elements
 

6. 

A particle that moves around the nucleus is _____.
a.
an electron
b.
an ion
c.
a neutron
d.
a quark
e.
a proton
 

7. 

Elements in Groups 3 through 12 of the periodic table are called _____.
a.
isotopes
b.
metalloids
c.
metals
d.
noble gases
e.
transition elements
 

8. 

A certain atom has 26 protons, 26 electrons, and 30 neutrons. Its mass number is _____.
a.
26
b.
30
c.
52
d.
56
e.
82
 

9. 

At room temperature, most metals are _____.
a.
gases
c.
radioactive
b.
liquids
d.
solids
 

10. 

The process by which solid iodine particles change directly to a gas without first becoming a liquid is called _____.
a.
condensation
b.
evaporation
c.
ionization
d.
radioactivity
e.
sublimation
 

11. 

A term that means "salt former" is _____.
a.
allotrope
b.
fluoride
c.
ionic
d.
metal
e.
halogen
 

12. 

Substances that conduct an electric current only under certain conditions are most likely to be _____.
a.
metals
c.
noble gases
b.
metalloids
d.
nonmetals
 

13. 

Different forms of the same element that have different properties because of different atom arrangements are called _____.
a.
allotropes
b.
carbons
c.
graphites
d.
halogens
e.
silicons
 

14. 

An allotrope of carbon that is soft and can be used as a lubricant is _____.
a.
diamond
b.
graphite
c.
sand
d.
silicon
e.
quartz
 

15. 

An allotrope of carbon that is hard and is often used in jewelry is _____.
a.
diamond
b.
graphite
c.
quartz
d.
silver
e.
sand
 

16. 

Hydrogen is grouped with the alkali metals because it _____.
a.
does not readily form compounds
c.
is a gas
b.
has one electron in its outer energy level
d.
is a metal
 

17. 

A chemical family whose members exist as diatomic molecules in the gaseous phase is the _____.
a.
actinide series
c.
halogens
b.
alkali metals
d.
lanthanide series
 

18. 

When hydrogen reacts with the active metals, it forms a chemical bond by _____.
a.
gaining one electron
c.
losing two electrons
b.
losing one electron
d.
sharing electrons
 

19. 

The elements in Groups 3-12 of the periodic table are the _____.
a.
actinides
b.
alkaline earth metals
c.
alkali metals
d.
halogens
e.
transition elements
 

20. 

A family of elements that has two electrons in its outer energy level is the _____.
a.
actinides
b.
alkaline earth metals
c.
alkali metals
d.
halogens
e.
transition elements
 

21. 

Metals can be used as wire because they are _____.
a.
alloys
c.
malleable
b.
ductile
d.
shiny
 

22. 

Elements in which the outer electrons are NOT held tightly are most likely to form _____ bonds.
a.
covalent
c.
metallic
b.
hydrogen
d.
radioactive
 

23. 

Bromine is the only halogen and nonmetal that is normally a _____.
a.
gas
c.
semiconductor
b.
liquid
d.
solid
 

24. 

The only metal that is a liquid at room temperature is _____.
a.
copper
b.
mercury
c.
silver
d.
sodium
e.
zinc
 

25. 

A synthetic element that is used in smoke detectors is _____.
a.
aluminum
c.
sodium
b.
americium
d.
technetium
 

26. 

All synthetic elements are _____.
a.
liquids
c.
radioactive
b.
needed by the human body
d.
useful in making plastics
 

27. 

Cobalt, iron, and nickel are metallic transition elements that are _____.
a.
gases
c.
magnetic
b.
liquids
d.
radioactive
 

28. 

Three transition elements in Group 12 of the periodic table are _____.
a.
copper, silver, and gold
c.
mercury, zinc, and cadmium
b.
iron, nickel, and cobalt
d.
neon, helium, and xenon
 

29. 

Any element with an atomic number greater than that of uranium is a _____.
a.
halogen
c.
transition element
b.
lanthanide
d.
transuranium element
 

30. 

The only noble gas with fewer than eight electrons in its outer level is _____.
a.
helium
c.
radium
b.
neon
d.
xenon
 

31. 

Elements that lie along the stair-step line of the periodic table are _____.
a.
liquids
c.
metalloids
b.
metals
d.
radioactive
 

32. 

The appearance of solid metals can be described as _____.
a.
dull
c.
powdery
b.
glassy
d.
shiny
 

33. 

A family of elements that contains the most reactive metals is the _____.
a.
actinides
b.
alkaline earth metals
c.
alkali metals
d.
transition elements
e.
noble gases
 

34. 

Synthetic elements comprise a majority of the _____.
a.
actinides
b.
halogens
c.
lanthanides
d.
oxides
e.
noble gases
 

35. 

In a chemical formula, the ratio of atoms in the compound is shown by numbers called _____.
a.
hydrates
b.
chemical symbols
c.
oxidation numbers
d.
subscripts
e.
superscripts
 

36. 

A group of atoms that acts together as one charged atom is a _____.
a.
crystal
c.
negative ion
b.
molecule
d.
polyatomic ion
 

37. 

The elements that make up a compound and the ratios of the atoms of those elements can be shown in a _____.
a.
chemical formula
c.
subscript
b.
chemical symbol
d.
superscript
 

38. 

A chemical bond that occurs when atoms share electrons is _____ bond.
a.
a covalent
c.
a magnetic
b.
an ionic
d.
a polyatomic
 

39. 

The name given to the combining ability of an atom is _____.
a.
atomic mass
c.
ionic number
b.
atomic number
d.
oxidation number
 

40. 

The sum of the oxidation numbers in a neutral compound is _____.
a.
a negative number
c.
a positive number
b.
one
d.
zero
 

41. 

The oxidation number of an atom is shown with a _____.
a.
negative number
c.
subscript
b.
positive number
d.
superscript
 

42. 

Which of the following correctly shows the formula for a hydrate?
a.
H2O
c.
MgSO4(H2O)7
b.
H2O2
d.
MgSO4 · 7H2O
 

43. 

How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable?
a.
2
b.
4
c.
6
d.
8
e.
10
 

44. 

What kind of chemical bond is formed when electrons are transferred from atom to atom?
a.
covalent
c.
ionic
b.
hydrate
d.
magnetic
 

45. 

What is the total number of atoms in the compound Ca(ClO3)2?
a.
2
b.
3
c.
5
d.
6
e.
9
 

46. 

How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2?
a.
3
b.
4
c.
7
d.
11
e.
12
 

47. 

What is the name of the compound with the formula NaCl?
a.
chlorine sodiate
c.
sodium chloride
b.
sodium chlorate
d.
sodium dichloride
 

48. 

Why do the noble gases NOT form compounds readily?
a.
They have empty outer energy levels.
b.
They have no electrons.
c.
They have seven electrons in the outer energy levels.
d.
Their outer energy levels are completely filled with electrons.
 

49. 

What is the ratio of potassium atoms to oxygen atoms in a binary compound made from these two elements?
a.
1:1
b.
1:2
c.
1:3
d.
2:1
e.
3:1
 

50. 

What is the name of a binary compound made up of lithium and chlorine?
a.
chlorine lithiate
c.
lithium chloride
b.
chlorine lithium
d.
lithium chlorate
 

51. 

Which of the following is the correct formula for magnesium nitrate?
a.
MgNO3
c.
Mg(NO3)2
b.
Mg2NO3
d.
Mg2(NO3)2
 

52. 

What is the charge of phosphate in K3PO4?
a.
7-
b.
3-
c.
1+
d.
5+
e.
4+
 

53. 

What is the correct name for K2SO4?
a.
potassium disulfide
c.
potassium sulfide
b.
potassium sulfate
d.
potassium(II) sulfate
 

54. 

What is the correct formula for magnesium oxide?
a.
MgO
c.
Mg2O2
b.
MgO2
d.
Mg2O
 

55. 

Using other insects to eat harmful insects is a safe alternative to _____.
a.
herbicides
c.
Freon
b.
insecticides
d.
disinfectants
 

Matching
 
 
Match each of the families listed below with the types of elements each contains. Each answer can be used more than once.
a.
metal
b.
nonmetal
c.
metalloid
d.
diatomic molecular
e.
metal, nonmetal, metalloid
f.
metal, nonmetal, metalloid, diatomic molecular
g.
metal, metalloid
h.
nonmetal, metalloid, diatomic molecular
 

56. 

alkali metal
 

57. 

alkaline earth metal
 

58. 

iron triad
 

59. 

halogens
 

60. 

noble gases
 

61. 

boron group
 

62. 

carbon group
 

63. 

nitrogen group
 

64. 

oxygen group
 

Problem
 

65. 

Suppose that you have just discovered a new element and have named it neptunite. While studying your new element, you find that it has two isotopes—neptunite-220 and neptunite-250. What is the average atomic mass of your new element? (Assume that these two isotopes are present in equal amounts in nature.)
 

66. 

Assume that an element is composed of one isotope with a mass of 142 and another isotope with a mass of 145. For each atom with a mass of 142, there are three atoms with a mass of 145. What is the average atomic mass of the element?
 



 
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