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Chemistry Sem 2 Final Study

Total questions: 100

Worksheet time: 2hrs 48mins

Name
Class
Date
1.

Discovered the neutron

a)

Ernest Rutherford

b)

James Chadwick

c)

J.J. Thomson

d)

John Dalton

2.
Which scientist saw the atom as a positively charged sphere with negative particles (electrons) embedded within?
a)
J.J. Thomson
b)
Niels Bohr
c)
John Dalton
d)
Ernest Rutherford
3.
Which scientist proposed a model of the atom in which the electrons are orbiting at different levels?
a)
Niels Bohr
b)
James Chadwick
c)
John Dalton
d)
Ernest Rutherford
4.
Which scientist used his gold foil experiment to show that an atom has a small, central, positively charged nucleus that contains most of the atom's mass?
a)
Rutherford
b)
Bohr
c)
Thomson
d)
Dalton
5.
Whose model of an atom is displayed in the picture?
a)
Thomson
b)
Rutherford
c)
Dalton
d)
Bohr
6.

Protons are located in the nucleus of the atom. A proton has

a)

No charge

b)

A negative charge

c)

A positive and a negative charge

d)

A positive charge

7.

Neutrons are in the nucleus of the atom. A neutron has

a)

A positive charge

b)

No charge

c)

A negative charge

d)

Twice as much positive charge as a proton

8.

Electrons are found in the nucleus of an atom.

a)

True

b)

False

9.

The periodic table shows that a carbon atom has six protons. This means that a carbon atom also has

a)

Six electrons

b)

Six neutrons

c)

More protons than electrons

d)

An atomic mass that equals six

10.

Neutrons and electrons are attracted to one another.

a)

True

b)

False

11.
Atoms are made up of three basic parts, which are -
a)
Protons, neutrons, electrons
b)
neutrinos, protons, neutrons
c)
quarks, protons, electrons
d)
electrons, neutrons, and quarks
12.

The atomic number of an atom is

a)

The mass of the atom

b)

The number of protons added to the number of neutrons

c)

The number of protons

d)

Negatively charged

13.

Because a few alpha particles bounced back from the foil, Rutherford concluded that they were

a)

striking electrons.

b)

magnetic.

c)

repelled by densely packed regions of positive charge.

14.

The observation that most alpha particles passed straight through an atom of gold lead Rutherford to conclude

a)

that the atom was mostly empty space.

b)

that the atom contained a large nucleus.

c)

that the atom had a positively charged nucleus.

15.

Isotopes are atoms of the same element that have different

a)

numbers of protons.

b)

masses.

c)

numbers of electrons.

16.

An atom is electrically neutral because

a)

the numbers of protons and neutrons are equal.

b)

the numbers of protons and electrons are equal.

c)

neutrons balance the protons and electrons.

17.

In Rutherford's experiments, most of the particles

a)

were absorbed by the foil.

b)

passed through the foil.

c)

combined with the foil.

18.
Rutherford concluded that the atom
a)
has a nucleus with a positive charge
b)
has a nucleus with a negative charge 
c)
is a small mass with negative and positive charges
d)
contains a nucleus without a charge
19.
This contains most of the mass of an atom
a)
Electron Cloud
b)
Nucleus
c)
Electron
20.
Contributes basically no mass to an atom.
a)
protons
b)
neutrons
c)
electrons
d)
protons and neutrons
21.
Atoms of the same element that have different number of neutrons are called 
a)
ions 
b)
atoms 
c)
isotopes
d)
elements 
22.
What is the mass number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
23.
This is the simplest of all atoms and contains only one proton and one electron
a)
Oxygen
b)
Hydrogen
c)
Water
24.
All matter is made of what?
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
25.

Who stated that all atoms of the same element are excacty alike?

a)

Democritus

b)

Dalton

c)

Thomson

d)

Bohr

26.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
27.

An atom's overall charge is ________.

a)

positive

b)

massive

c)

neutral

d)

negative

28.
Who came up with this model of an atom?
a)
J.J. Thompson
b)
Ernest Rutherford
c)
Neils Bohr
d)
James Chadwick
29.
The atomic number for Oxygen is 8, so
a)
there are 8 protons in the atom
b)
the atomic mass is less than 8
c)
the mass of the atom is 8
d)
the atom is decaying
30.

Who would have said, "An Atom is a tiny, invisible, indestructible and an empty sphere."

a)

Dalton

b)

Bohr

c)

Thomson

d)

Rutherford

31.

Who would have said, "An atom is composed of a dense, positively charged nucleus. The electrons move in circular orbits at fixed distances from the nucleus."

a)

Dalton

b)

Bohr

c)

Thomson

d)

Rutherford

32.

Who proposed the model in option "B"?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

33.

One of the first people to state that matter is made up of atoms was

a)

Democritus.

b)

Aristotle.

c)

Dalton.

d)

Rutherford.

34.

Dalton's model of an atom is best described as

a)

a solar system.

b)

a solid sphere.

c)

a plum pudding.

d)

an electron cloud.

35.

Who provided the first evidence that atoms contain subatomic particles?

a)

Dalton

b)

Rutherford

c)

Thomson

d)

Bohr

36.

Which particle is the least massive?

a)

proton

b)

electron

c)

neutron

d)

nucleus

37.

All atoms of an element have the same

a)

mass number.

b)

number of isotopes.

c)

atomic number.

d)

number of neutrons.

38.

The number of neutrons in an atom equals the

a)

mass number minus atomic number.

b)

atomic number plus number of electrons.

c)

mass number plus atomic number.

d)

atomic number minus mass number.

39.

The atomic number of sulfur is 16. How many electrons are there in an atom of sulfur-34 ?

a)

16

b)

18

c)

34

d)

50

40.

The only woman scientist known to have contributed to atomic theory was

a)

Rosalind Franklin

b)

Henrietta Lacks

c)

Frida Kahlo

d)

Marie Curie

41.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
42.

What shape is the s orbital?

a)

sphere

b)

dumbbell

c)

double dumbbell

d)

very complex shape

43.

When l=0, we call it the ___ orbital. When l=1, it is the ___ orbital. When l = 2, it is the ___ orbital and when l = 3, it is the ___ orbital.

a)

s, p, d, f

b)

a, b, c, d

c)

l, m ,n, o

d)

w, x, y, z

44.

What is the spin quantum number refer to?

a)

the main energy level

b)

the shape of the orbital

c)

the orientation of the orbital

d)

the spin of the electrons

45.

What does the letter (l) stand for?

a)

principal quantum number

b)

angular momentum quantum number

c)

magnetic quantum number

d)

spin quantum number

46.

What is the magnetic quantum number refer to?

a)

the main energy level

b)

the shape of the orbital

c)

the orientation of the orbital

d)

the spin of the electrons

47.

What is the angular momentum quantum number refer to?

a)

the main energy level

b)

the shape of the orbital

c)

the orientation of the orbital

d)

the spin of the electrons

48.

What is the principal quantum number refer to?

a)

the main energy level

b)

the shape of the orbital

c)

the orientation of the orbital

d)

the spin of the electrons

49.

No two electrons can have the same four quantum numbers.

a)

TRUE

b)

FALSE

50.

Which values can (n) be?

a)

only 0

b)

0, 1, 2, 3...

c)

1,2,3,4...

d)

-2 < n < +2

51.

What values of ml can there be if l = 2 (d orbital)?

a)

0

b)

-1 to +1

c)

-2 to +2

d)

-3 to +3

52.

Name the element- 1s2 2s2 2p6 3s2 3p6 4s2 3d5

a)

Manganese

b)

Magnesium

c)

Aluminum

d)

Boron

53.

Name the element. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

a)

Gallium

b)

Indium

c)

Aluminum

d)

Germanium

54.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
55.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
56.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
57.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
58.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
59.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
60.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
61.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
62.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
63.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
64.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
65.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
66.

The horizontal row on the periodic table is called a

a)

group

b)

family

c)

period

d)

atomic number

67.

A vertical column is called...

a)

group

b)

tower

c)

period

d)

crew

68.

Most of the elements on the periodic table are classified as _____.

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Periods

69.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
70.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
71.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
72.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
73.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
74.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
75.
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 nuetrons
76.
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.
77.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
78.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
79.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
80.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

a)

decreases, increases

b)

increases, increases

c)

increases, decreases

d)

stays the same, increases

81.

Noble gases are characterized as having

a)

partially filled outermost energy levels

b)

completely filled outermost energy levels

c)

electrons in the d and f sublevels

d)

high reactivity

82.

Valence electrons are:

a)

Electrons in the highest energy level

b)

Electrons closest to the nucleus

c)

Electrons that just come and go - they don't stay with the atom

d)

Electrons that are excited

83.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-5
d)
1-20
84.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
85.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
86.
When dissolved in water, bases produce:
a)
acids
b)
salts
c)
hydrogen ions
d)
hydroxide ions
87.

Ammonia (NH3) only partially dissociates into ions in water. This makes it a...

a)

strong acid

b)

weak acid

c)

weak base

d)

strong base

88.

Sodium hydroxide (NaOH) dissociates completely in water producing a high concentration of hydroxide ions. This makes it a...

a)

Acid

b)

Strong base

c)

Weak base

d)

Strong acid

89.

Hydroxides like KOH and Ca(OH)2 dissociate easily and completely in water making them...

a)

strong acids

b)

weak acids

c)

weak bases

d)

strong bases

90.
Which accepts protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
91.

An acid that very easily and completely ionizes when it dissolves in water is a...

a)

strong acid

b)

weak acid

c)

weak base

d)

strong base

92.
The hydroxide ion is a soft drink is 5.00 x 10-12 M.  Find the pH.
a)
0.002
b)
2.7
c)
11.3
d)
14
93.
What is the hydrogen ion concentration in a solution with pOH = 3.3?
a)
10.7 M
b)
0.00050 M
c)
0.000025 M
d)
2.0 x 10-11 M
94.
I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need?
a)
2.5mL
b)
5mL
c)
25mL
d)
50mL
95.
What is the [OH-] if the [H+] is 1.0 x 10-3M?
a)
1.0 x 10-3 M
b)
6.02 x 10-23 M
c)
1.0 x 10-14 M
d)
1.0 x 10-11 M
96.

What is the conjugate base of HClO4?

a)

H+

b)

Cl-

c)

ClO3-

d)

ClO4-

97.

Acetic Acid is a weak monoprotic acid. It's concentration is 0.20M and it's equilibrium concentration of H+ ions is 0.0019M. Calculate it's Ka value.

a)

1.8x10 -5

b)

1.8x10 -15

c)

.0019

d)

5.56x10 -10

98.

Gallic Acid is a weak monoprotic acid. It's concentration is 0.280M and it's equilibrium concentration of H+ ions is 0.0033M. Calculate it's pH value.

a)

3.9x10 -5

b)

4.96

c)

2.48

d)

.280

99.

pH is mathematically defined as the "negative of the base ten logarithm of the ___"

a)

molar mass of protons

b)

concentration of hydrogen ions in solution

c)

mass of hydrogen ions in solution

d)

molarity of helium ions

100.

What symbol is used for the water dissociation constant?

a)

Cw

b)

Wc

c)

Kw

d)

Wk

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