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Finals Review

Total questions: 49

Worksheet time: 39mins

Name
Class
Date
1.

What is the name of the change of state where a gas becomes solid without first becoming liquid

a)
sublimation
b)
deposition
c)
vaporization
d)
evaporation
2.

What particle number is equal to the atomic number (Z)

a)

Protons

b)

Electrons

c)

Neutrons

3.

What is the charge of a neutron?

a)

Negative

b)

Positive

c)

Neutral

4.

Which statement is correct for the ion shown?

a)

The ion contains 15 subatomic particles in the nucleus.

b)

The ion contains more protons than neutrons in the nucleus.

c)

The ion has an electron arrangement of 1s2 2s2

d)

Most of the total volume of the ion is empty space.

5.

A sample of zinc has the following composition:

What is the relative atomic mass of the zinc in this sample?

a)

64.5

b)

65.0

c)

65.9

d)

66.4

6.

Which of the following elements is a metalloid?

a)

Hydrogen

b)

Helium

c)

Chromium

d)

Astatine

7.
The MOST electronegative element is ____.
a)
Helium
b)
Hydrogen
c)
Fluorine
d)
Francium
8.
Which of the following will have a larger radius than Zinc (Zn)?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
9.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
10.

Which trends are correct across period 3 (from Na to Cl)?

I. Atomic radius decreases II. Melting point increases III. First ionization energy increases

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

11.

‘Bronze is harder than copper’. Which of the following is the best to explain the statement?

a)

Atoms in bronze are arranged closely packed and less empty spaces.

b)

Layers of atoms in bronze are not easily slide over each other.

c)

Atomic size of copper and tin is different.

d)

Bronze is a mixture of copper and tin

12.
Which element has a noble gas configuration of [Ne] 3s2 3p3?
a)
Magnesium
b)
Phosphorus
c)
Aluminum
d)
Sulfur
13.
Which element has the following electron configuration: [Ar] 4s2 3d10 4p4?
a)
Bromine
b)
Gold
c)
Iodine
d)
Selenium
14.
Which statement describes the general trends in electronegativity and metallic properties across Period 3 moving from left to right? 
a)

Electronegativity increases and metallic properties (character) decrease.

b)

Electronegativity decreases and metallic properties (character)increase.

c)

Both electronegativity and metallic properties increase.(character)

d)

Both electronegativity and metallic properties decrease.(character)

15.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting and it conducts electricity when liquid

c)

A high boiling point and it conducts electricity when solid

16.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
17.

The number of electrons in the valence shell of elements A and B, are 6 and 7 respectively. What is the formula and type of bonding in a compound formed by these elements?

a)

A2B Covalent

b)

AB2 Covalent

c)

A2B Ionic

d)

AB2 Ionic

18.
Sublimation is
a)
when solid turns into gas
b)
when gas turns into plasma
c)
when liquid turns into gas
d)
when gas turns into solid
19.

Which equation represents the sublimation of carbon dioxide?

a)

CO2 (g) → CO2 (s)

b)

CO2 (s) → CO2 (g)

c)

CO2 (g) → CO2 (l)

d)

CO2 (l) → CO2 (g)

20.

 Which experimental results support the theory that electrons exist in discrete energy levels?

a)

NMR

b)

X-Ray diffraction

c)

Emission Spectra

d)

IR Spectra

21.

The composition of this substance is uniform throughout

a)

Homogenous mixtures

b)

Heterogeneous misxtures

c)

Elements

d)

Compounds

22.

Ionization energy increases

a)

from L to R and from bottom to top in the periodic table

b)

from L to R and from top to bottom in the periodic table

c)

from R to L and from bottom to top in the periodic table

d)

from R to L and from top to bottom in the periodic table

23.

Which combination would create the strongest ionic bond?

a)

Large ionic radius

High charge on ions

b)

Small ionic radius

High charge on ions

c)

Large ionic radius

Low charge on ions

d)

Small ionic radius

Low charge on ions

24.

Describe the state of the substance at letter A. (a)  

Choose from the below words
Solid
Liquid
Melting
Evaporating
25.

Which letter indicates where water is in both the solid and liquid phase at the same time?

a)

A

b)

B

c)

C

d)

D

e)

E

26.
1.  What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
27.

Which species has the same electron configuration as Neon?

a)

Cl-

b)

O

c)

Na+

d)

P3-

28.

Which periodic trend is described correctly?

a)

A

b)

B

c)

C

d)

D

29.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
30.

In order to go from ground state to an excited state, an electron must

a)

emit energy

b)

absorb energy

c)

wiggle

31.

When an electron returns to ground state from an excited state, the atom will (a)  

Choose from the below words
emit energy
absorb energy
rotate
wiggle
32.

Which block of elements are known as transition elements?

a)

p-block

b)

s-block

c)

d-block

d)

f-block

33.
How many significant figures does the following number have?
0.00345
a)
6
b)
5
c)
3
d)
Ambiguous: 3,4,5, or 6
34.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
35.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
36.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
37.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
38.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
39.

Which type of bonding involves positive ions surrounded by a sea of mobile electrons?

a)

metallic bonds

b)

polar covalent bonds

c)

nonpolar covalent bonds

d)

ionic bonds

40.

Which compound contains ionic bonds?

a)

NaH

b)

CH4

c)

H2O

d)

C6H12O6

41.

What kind of mixture is shown in the picture?

a)

Homogeneous

b)

Heterogeneous

42.

How many protons does indium have?

a)

49

b)

66

c)

114

d)

115

43.

How many valence electrons does Lithium (Li) have?

a)

8

b)

1

c)

5

d)

2

44.

  How do the following properties change down Group 17 of the periodic table?

a)

A

b)

B

c)

C

d)

D

45.

Describe the electron arrangement arround the central atom.

a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number electrons

46.

What is the shape of carbon dioxide (CO2)?

a)

Tetrahedral

b)

Trigonal Planar

c)

Linear

d)

Bent

47.

What is the shape of boron trihydride (BH3)?

a)

Trigonal Planar

b)

Bent

c)

Linear

d)

Tetrahedral

48.

What is the shape of methane (CH4)?

a)

Linear

b)

Trigonal Planar

c)

Bent

d)

Tetrahedral

49.

How many electrons would a Nitrogen ion gain/lose? If it has 5 valence electrons.

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

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