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Extra credit review first six weeks

Total questions: 46

Worksheet time: 46mins

Name
Class
Date
1.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
2.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
3.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
4.
What element has the valence shell configuration
3s2 3p2
a)
Al
b)
B
c)
Si
d)
Ga
5.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
6.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
7.
Positive ions form when atoms _________ valence electrons.
a)
lose
b)
gain
c)
share
d)
gain or share
8.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
9.
What charge does an atom have if it LOSES an electron? 
a)
Positive (+)
b)
Negative (-)
10.
What is the number of protons?
a)
34
b)
16
c)
18
d)
S
11.
What is the number of neutrons?
a)
34
b)
79
c)
45
d)
35
12.

Identify the type of reaction.
AB →\rightarrow A + B

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

13.

Identify the type of reaction shown.
A + B →\rightarrow AB

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

14.
Which generalized equation represents a synthesis reaction?
a)
A + BC → AC+ B
b)
A + B → AB
c)
AB → A + B
15.
Which generalized equation represents a single displacement reaction?
a)
A + BC → AC+ B
b)
A + B → AB
c)
AB → A + B
16.
Which generalized equation represents a decomposition reaction?
a)
A + BC → AC+ B
b)
A + B → AB
c)
AB → A + B
17.

How can electronegativity values predict the type of bond between two elements?

a)

Measuring the boiling point of the elements

b)

Comparing the electronegativity difference between two elements.

c)

Counting the number of valence electrons in the elements

d)

Looking at the atomic number of the elements

18.

Do noble gases have electronegativity values?

a)

yes

b)

no

19.

Why does electronegativity decrease as you go down a group?

a)

As you go down a group, the outer electrons are further away from the nucleus

b)

As you go down a group, the nucleus is less able to attract electrons in a bond

c)

Both of these

d)

None of these

20.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

21.

Electronegativity (a)   as you go down a group.

22.

Which element has a lower electronegativity value?

a)

Calcium

b)

Barium

23.

Ionic bonds form by __________.

a)

sharing electrons

b)

attraction between opposite charges

c)

delocalized electrons

d)

electron spins

24.

Is KCl an ionic or covalent bond?

a)

ionic

b)

covalent

25.

How do covalent bonds form?

a)

sharing electrons

b)

attraction between opposite charges

c)

delocalized electrons

d)

electrons spinning

26.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

27.

What must the difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

28.
Which element does this structure represent?
a)
Lithium
b)
Helium
c)
Scandium
d)
Fluorine
29.
What group does this element belong to?
a)
Group 1: Alkali metals
b)
Group 18: Noble Gases
c)
Group 2: Alkaline-Earth Metals
d)
Group 17: Halogens
30.

What will be the charge of a bromine ion?

a)

+7

b)

-7

c)

-1

d)

+1

31.

Which of the following is a covalent bonding?

a)

MgS

b)

NaCl

c)

CH4

d)

LiBr

32.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
33.

A group of friends gather around a fire to stay warm. This is an example of ________.

a)

conduction

b)

convection

c)

radiation

34.

In heat transfer, heat always flows from the _______________ substance to the _______________ substance.

a)

hotter to colder

b)

colder to hotter

c)

hotter to hotter

d)

colder to colder

35.

Which is an example of heat being transferred by conduction?

a)

a furnace heating the air in a school

b)

an ice cube melting in a person’s hand

c)

a pot of water on a stove boiling

d)

the sun heating water in a swimming pool

36.

Near the ceiling of a room the air is warmer. The warm air rises because of ________.

a)

conduction

b)

convection

c)

radiation

37.

Hot coffee is stirred with a spoon; the spoon gets hot due to ________.

a)

conduction

b)

convection

c)

radiation

38.

The type of heat transfer that creates currents in water is called ________.

a)

conduction

b)

convection

c)

radiation

39.
If an atom becomes an ion with a 2+ charge, what does that mean?
a)
It has lost 2 electrons
b)
It has gained 2 electrons
c)
The atom is in period 2
d)
The atom has an atomic # of 2
40.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
41.
Which of these combinations is an ionic compound made of?
a)
Metal and Metal
b)
Nonmetal and Nonmetal
c)
Metal and Nonmetal
d)
Cation and Cation
42.
The name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
43.

What is the correct name of the compound P2O5

a)

phosphorous oxide

b)

diphosphorous pentoxide

c)

phosphorous pentoxide

44.

What formula represents dinitrogen trioxide?

a)

N3O2

b)

NO2

c)

N2O3

45.

What is the name of the compound P4S10

a)

phosphorous sulfide

b)

tetraphosphide decasulfate

c)

phosphorous decasulfate

d)

tetraphosphorous decasulfide

46.
What is the proper name for CaCl2?
a)
Calcium dichloride
b)
Monocalcium dichloride
c)
Calcium chloride
d)
Calcium chlorine

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