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CBA 01 Review (TEKS 5A-8B)

Total questions: 66

Worksheet time: 1hrs 3mins

Name
Class
Date
1.
How many significant figures does the following number have?
0.00345
a)
6
b)
5
c)
3
d)
Ambiguous: 3,4,5, or 6
2.
How many significant figures does the following number have: 100.00210
a)
7
b)
8
c)
10
d)
Ambiguous: 7 or 8
3.
Round 1289 to three significant figures
a)
1290
b)
130
c)
1300
d)
1.29x103
4.
Change from standard form to scientific notation: 12,000,000
a)
12.0  x  107
b)
0.12  x  107
c)
1.2  x  106
d)
1.2  x  107
5.
Change from standard form to scientific notation:  0.000398
a)
39.8  x  10-5
b)
3.98  x  10-5
c)
3.98  x  10-4
d)
39.8  x  10-6
6.
Change from standard form to scientific notation: 0.004078
a)
4.078  x  10-3
b)
4.078  x  103
c)
40.78  x  10-4
d)
.4078  x  10-2
7.

Dmitri Mendeleev arranged the 63 known elements at the time by __________________.

a)

atomic number

b)

atomic mass

c)

neutron number

d)

none of the above

8.

Why did Dmitri Mendeleev leave spaces in his periodic table?

a)

He left spaces for undiscovered elements.

b)

He left spaces for discovered elements.

c)

He left spaces to be more organized.

d)

none of the above

9.

The modern periodic table is arranged by ___________________.

a)

atomic number

b)

atomic mass

c)

neutrons only

d)

none of the above

10.

Alkali Metals are ______

a)

in group 1 and are the most reactive metals.

b)

in group 2 and are the second most reactive metals.

c)

in group 17 and are the most reactive nonmetals.

d)

in group 18 and are inert (unreactive).

11.

Match the following

a)

in group 1 and are the most reactive metals.

1.

Alkali Metals

b)

In group 2 and are the second most reactive metals.

2.

Alkaline Earth Metals

c)

In group 17 and are the most reactive nonmetals..

3.

Halogents

d)

Complete, Stable!

4.

Noble Gases

e)

Metallic elements that have valence electrons in two shells instead of only one.

5.

Transition Metals

12.

What group is carbon in?

a)

1

b)

2

c)

13

d)

14

e)

15

13.

What are the vertical columns on the periodic called?

a)

groups

b)

periods

c)

nonmetals

d)

metals

e)

metalloids

14.

How do you calculate the number of neutrons? *

a)

Mass = Atomic number - Neutrons

b)

Mass - Atomic number = Neutrons

c)

Atomic number = Neutrons

15.

How many valence electrons does the element have?

a)

1

b)

2

c)

3

d)

4

16.

Who discovered the Law of Octaves?

a)

Henry Moseley

b)

Lothar Meyer

c)

Antoine Lavoisier

d)

John Newlands

17.

He classified some elements into groups of three, which he called triads.

a)

John Newlands

b)

Johann Wolfang Döbereiner

c)

Antoine Lavoisier

d)

Lothar Meyer

18.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of neutrons in the nucleus

c)

the number of protons and neutrons in the nucleus

d)

the number of protons in the energy levels

19.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of neutrons in the nucleus

c)

the number of protons and neutrons in the nucleus

d)

the number of protons and electrons in the atom

20.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

21.

Explain how the Rutherford gold foil experiment correctly advanced atomic theory away from the plum pudding mode

a)

it proved the atom contained positive AND negative charges.

b)

It proved the positive charge is concentrated in a relatively small region of the atom.

c)

It proved the atom contains protons, electrons, and neutrons.

d)

It proved that atoms are spherical in shape and not shaped like pudding

22.

The nucleus of an atom contains (a)   and neutrons

23.

What did Bohr's atomic theory model look like?

a)

A ring with gold foil in the middle.

b)

Electrons orbiting the nucleus like the planets around the sun.

c)

A cloud of electrons floating around the nucleus.

d)

A scoop of chocolate chip ice cream. It had electrons scattered within a ball of positive charge.

24.

What did Rutherford discover about atoms?

a)

An atom is always negatively charged.

b)

An atom is mostly empty space, but has a dense positively charged center(nucleus).

c)

An atom is always positively charged.

d)

All particles will pass straight through gold foil with no change in path.

25.
Select the correct order of waves on the EMS 
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
26.
The blue section of the wave is measuring .
(a)  
Choose from the below words
wavelength
crest
trough
amplitude 
27.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

28.

Isotopes of an element have a different number of (a)  

29.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

30.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

31.

There are two primary isotopes found in any sample of copper: copper-63 and copper-65. The isotope 65Cu composes 69.2% of the sample and 63Cu comprises the other 30.8%. Based on this data, what is the atomic mass of copper?

a)

29 amu

b)

63.546 amu

c)

64.4 amu

d)

63.6 amu

32.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

33.

How many valence electrons should Magnesium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

34.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

35.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
36.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
37.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
38.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
39.

What is the maximum number of electrons that an S orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

40.
Has a mass of 4 and a charge of +2
a)
Alpha
b)
Beta
c)
Gamma
41.
Has the symbol
a)
Alpha
b)
Beta 
c)
Gamma
42.
Takes two small nuclei and combines them into a larger nucleus
a)
fission
b)
fusion
43.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
44.
Which type of nuclear radiation is being emitted here?
a)
alpha
b)
beta
c)
gamma
d)
none
45.

When lithium and oxygen bond the formula is

a)

LiO

b)

OiL

c)

Li2O

d)

LiO2

46.

What is the correct formula for strontium nitride

a)

SrN

b)

Sr3N2

c)

Sr2N3

d)

N3Sr2

47.

What is the correct formula for aluminum fluoride

a)

AlF

b)

AlF2

c)

Al3F

d)

AlF3

48.

What is the IUPAC name for FePO4

a)

iron phosphite

b)

iron (III) phosphite

c)

iron (III) phosphate

d)

iron (II) phosphite

49.

What is the chemical formula for disulfur trioxide

a)

S3O2

b)

SO

c)

S2O3

d)

S2O

50.

What is the chemical formula for octanitrogen tetraoxide

a)

N8O3

b)

N7O3

c)

N8O3

d)

N8O4

51.

What is the chemical name for P4H7

a)

tetraphosphorus heptahydrogide

b)

phosphorus heptahydride

c)

tetraphosphorus heptahydride

d)

tetraphosphorus heptahydrogen

52.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
53.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
54.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
55.
What are ionic bonds?
a)
Valence electrons transferred between atoms
b)
Inner most electrons transferred between atoms
c)
Sharing electrons
56.
Ionic bonds occur between...
a)
A metal and a nonmetal
b)
Two metals
c)
Two nonmetals
d)
Two gases
57.
What bond involves the sharing of electrons?
a)
Ionic
b)
Transitive
c)
Covalent
58.

Valence electrons are found

a)

in the innermost energy level of an atom

b)

in the middle energy levels of an atom

c)

in the outermost energy levels of an atom

59.

What is the molar mass of Cl2?

a)

17 g/mol

b)

35.5 g/mo;

c)

71.0 g/mol

d)

89 g/mol

60.

What id the molar mass of UF6?

a)

101 g/mol

b)

238 g/mol

c)

257 g/mol

d)

352 g/mol

61.

Calculate the molar mass of KOH.

a)

28 g/mol

b)

56 g/mol

c)

84 g/mol

d)

112 g/mol

62.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

63.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
64.
How many atoms of carbon are in 6.00g of carbon?
a)
1.20x1024atoms C
b)
6.02x1023atoms C
c)
3.01x1023atoms C
d)
1.50x1023atoms C
65.
What is the mass of 0.89 mol of CaCl2?
a)
111 grams
b)
0.008 grams
c)
98.9 grams
d)
none of the choices
66.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.05 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5 moles

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