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Gen Chem Midterm Review

Total questions: 105

Worksheet time: 26hrs 1mins

Name
Class
Date
1.

What is the branch of science that studies matter and its changes?

a)

Biology

b)

Chemistry

c)

Integrated Chemistry and Physics

d)

Anatomy/Physiology

2.

Which is a homogenous mixture

a)

A metal alloy

b)

water

c)

nitrogen gas

d)

concrete

3.

A compound is:

a)

two or more elements combined in a fixed ratio

b)

two or more elements

c)

an element

d)

a mixture

4.

In a chemical reaction, matter is :

a)

neither created nor destroyed

b)

created

c)

destroyed

d)

converted to energy

5.

In a chemical reaction, energy is :

a)

neither created nor destroyed

b)

created

c)

destroyed

d)

converted to matter

6.

Has a definite shape and volume

a)

solid

b)

liquid

c)

gas

d)

plasma

7.

Has a definite volume, but takes the shape of its container

a)

solid

b)

liquid

c)

gas

d)

plasma

8.

Does not have definite shape or volume

a)

solid

b)

liquid

c)

gas

d)

plasma

9.

If the components of a mixture retain their properties and are not evenly distributed, it is most likely a:

a)

homogenous mixture

b)

heterogenous mixture

c)

compound

d)

element

10.

The ability to react (undergo a chemical change) is a:

a)

Chemical property

b)

Physical property

c)

trait

d)

characteristic

11.

Can be observed or measured without changing the substance:

a)

Chemical property

b)

Physical property

c)

trait

d)

characteristic

12.

Chemistry with a specific goal or outcome:

a)

Applied chemistry

b)

Pure Chemistry

c)

General Chemistry

d)

Honors Chemistry

13.

Chemistry for the sake learning new things:

a)

Applied chemistry

b)

Pure Chemistry

c)

General Chemistry

d)

Honors Chemistry

14.

Matter with a uniform and definite composition:

a)

substance

b)

stuff

c)

matter

d)

mass

15.

An action that changes a substances identity:

a)

Chemical change

b)

Physical change

16.

An action that does not change a substances identity:

a)

Chemical change

b)

Physical change

17.

A measurement that is close to its accepted value is:

a)

Accurate

b)

Precise

c)

neither accurate nor precise

d)

both accurate and precise

18.

A measurement that is close to other values is:

a)

Accurate

b)

Precise

c)

neither accurate nor precise

d)

both accurate and precise

19.

How many sig figs are in the value 7538.002?

a)

4

b)

5

c)

6

d)

7

20.

How many sig figs are in the value 1001?

a)

4

b)

5

c)

6

d)

7

21.

Which digit in 534.6 is estimated or unknown?

a)

4

b)

5

c)

6

d)

3

22.

Round 543.28 to 2 significant figures

a)

540

b)

543

c)

54

d)

540.00

23.

How does the quantity being measured change when its multiplied by a conversion factor?

a)

It doesn't. Only the value changes.

b)

The quantity changes, but the value doesn't.

c)

Both the quantity and the value change.

d)

Nothing changes.

24.

Percent error calculations are always:

a)

Positive

b)

Negative

c)

Neutral

d)

Accepted - experimental

25.

878,000,000,000 can be written as:

a)

8.78 x 1011

b)

8.78 x 1012

c)

8.78 x 10-11

d)

87.8 x 1010

26.

2.98 x 10-9 equals

a)

2,980,000,000

b)

0.00000000298

c)

0.0000000298

d)

298,000,000

27.

Mass number equals

a)

number of protons

b)

number of neutrons

c)

protons + neutrons

d)

protons + electrons

28.

Gold has a mass number of 197 amu and an atomic number of 79. It has:

a)

79 neutrons

b)

197 electrons

c)

118 neutrons

d)

197 protons

29.

The man who proposed the first atomic idea was:

a)

Democritus

b)

Thomson

c)

Dalton

d)

Rutherford

30.

The man who proposed the first atomic theory was:

a)

Democritus

b)

Thomson

c)

Dalton

d)

Rutherford

31.

The man who discovered the electron and proposed the plum pudding model was:

a)

Democritus

b)

Thomson

c)

Dalton

d)

Rutherford

32.

The man who conducted the gold foil experiment, discovered the nucleus, and proposed the nuclear model was:

a)

Democritus

b)

Thomson

c)

Dalton

d)

Rutherford

33.

Why are atomic masses and mass numbers given in amu's?

a)

They're more convenient to work with than actual atomic masses.

b)

They're more accurate than actual atomic masses.

c)

They're more flexible than actual atomic masses.

d)

Actual atomic masses are too small to be measured.

34.

Positive (+1) subatomic particle with a mass of 1 amu

a)

proton

b)

neutron

c)

electron

d)

atom

35.

Neutral (0) subatomic particle with a mass of 1 amu

a)

proton

b)

neutron

c)

electron

d)

atom

36.

Negative (-1) subatomic particle with a mass of 1/1840 amu

a)

proton

b)

neutron

c)

electron

d)

atom

37.

Which subatomic particles are found in the nucleus?

a)

protons

b)

neutrons

c)

protons and neutrons

d)

protons and electrons

38.

Every atom of an element has the same number of:

a)

protons

b)

neutrons

c)

electrons

d)

isotopes

39.

Average atomic mass is calculated by:

a)

summing the relative abundance x each isotope's mass

b)

protons + neutrons

c)

mass number - neutrons

d)

relative abundance times atomic number

40.

Isotopes of an element have:

a)

different numbers of neutrons

b)

different numbers of protons

c)

different numbers of electrons

d)

different atomic numbers

41.

S orbitals are shaped like a:

a)

sphere

b)

dumb bell

c)

4 leaf clover

d)

flower

42.

P orbitals are shaped like a:

a)

sphere

b)

dumb bell

c)

4 leaf clover

d)

flower

43.

D orbitals are shaped like a:

a)

sphere

b)

dumb bell

c)

4 leaf clover

d)

flower

44.

F orbitals are shaped like a:

a)

sphere

b)

dumb bell

c)

4 leaf clover

d)

flower

45.

Electrons enter the lowest energy levels first

a)

aufbau principle

b)

Pauli exclusion principle

c)

Hund's rule

46.

Paired electrons must have opposite spins

a)

aufbau principle

b)

Pauli exclusion principle

c)

Hund's rule

47.

Electrons occupy each orbital in the same direction before making pairs

a)

aufbau principle

b)

Pauli exclusion principle

c)

Hund's rule

48.

When an electron absorbs a quantum of energy:

a)

It goes up an energy level

b)

It emits a photon of light

c)

It absorbs a photon of light

d)

it doubles its energy

49.

The s sublevel can contain _____ orbitals.

a)

1

b)

3

c)

5

d)

7

50.

The p sublevel can contain _____ orbitals.

a)

1

b)

3

c)

5

d)

7

51.

The d sublevel can contain _____ orbitals.

a)

1

b)

3

c)

5

d)

7

52.

The f sublevel can contain _____ orbitals.

a)

1

b)

3

c)

5

d)

7

53.

Full and half-full orbitals are more:

a)

stable

b)

reactive

c)

volatile

d)

energetic

54.

The first principal energy level (n=1) contains:

a)

an s sublevel

b)

an s and p sublevel

c)

an s, p, and d sublevel

d)

an s, p, d, and f sublevel

55.

The second principal energy level (n=2) contains:

a)

an s sublevel

b)

an s and p sublevel

c)

an s, p, and d sublevel

d)

an s, p, d, and f sublevel

56.

The third principal energy level (n=3) contains:

a)

an s sublevel

b)

an s and p sublevel

c)

an s, p, and d sublevel

d)

an s, p, d, and f sublevel

57.

The fourth principal energy level (n=4) contains:

a)

an s sublevel

b)

an s and p sublevel

c)

an s, p, and d sublevel

d)

an s, p, d, and f sublevel

58.

The alkali metals and alkaline earth metals make up the _____ block

a)

s

b)

p

c)

d

d)

f

59.

The poor metals, metalloids, and nonmetals make up the _____ block.

a)

s

b)

p

c)

d

d)

f

60.

The transition metals make up the _____ block.

a)

s

b)

p

c)

d

d)

f

61.

The lanthanoid and actinoid series (aka inner transition metals) make up the _____ block.

a)

s

b)

p

c)

d

d)

f

62.

Who organized elements into triads?

a)

Moseley

b)

Mendeleev

c)

Dobereiner

d)

Seaborg

63.

Created the first "working" or "credible" periodic table; left blanks for undiscovered elements

a)

Moseley

b)

Mendeleev

c)

Dobereiner

d)

Seaborg

64.

Organized the periodic table by atomic number

a)

Moseley

b)

Mendeleev

c)

Dobereiner

d)

Seaborg

65.

Mendeleev organized his table by:

a)

atomic mass

b)

atomic radius

c)

atomic number

d)

electronegativity

66.

Synthesized many elements and contributed to the modern layout of the periodic table

a)

Moseley

b)

Mendeleev

c)

Dobereiner

d)

Seaborg

67.

A period is a:

a)

row

b)

column

c)

block

d)

triad

68.

A group is a:

a)

row

b)

column

c)

block

d)

triad

69.

Alkali metals are in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

70.

Alkaline earth metals are in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

71.

Halogens are in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

72.

Noble gases are in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

73.

Malleability is:

a)

The ability to bent or hammered into sheets

b)

The ability to be pulled into wires

c)

A property of nonmetals

d)

Luster

74.

Ductility is:

a)

The ability to bent or hammered into sheets

b)

The ability to be pulled into wires

c)

A property of nonmetals

d)

Luster

75.

"Shininess" is:

a)

The ability to bent or hammered into sheets

b)

The ability to be pulled into wires

c)

A property of nonmetals

d)

Luster

76.

An elements' valence electrons:

a)

Are its outermost electrons

b)

Determine its chemical behavior and bonding

c)

Are shown by its location on the periodic table

d)

all of the above

77.
energy required to remove an electron from gaseous elements
a)
ionization energy
b)
electronegativity
c)
octet rule
d)
periodic law
78.
indication of an atoms ability to attract electrons in a chemical bond
a)
electronegativity
b)
ionization
c)
periodic law
d)
transition elements
79.
elements in the same group have the same
a)
atomic radius
b)
energy level of outer electrons
c)
nuclear change
d)
number of valence electrons
80.
identify the period and group of the element that has the electron configuration [Ne]3s2 3p3
a)
period 2, group 2
b)
period 3, group 1
c)
period 3, group 13
d)
period 3, group 15
81.
what is the trend in atomic radii as you move from left to right across the period
a)
generally decreases
b)
generally increases
c)
remains the same
d)
various randomly
82.
the trend in the atomic radii as you move down the group 1 elements is partially due to
a)
decreased distance of outer electrons
b)
increased nuclear change
c)
increased number of electrons in outer energy level
d)
shielding by inner electrons
83.
How many electrons does an atom generally need in its outer level to be the most stable
a)
4
b)
8
c)
10
d)
12
84.
Which of these element is the least metallic?
a)
Potassium (K)
b)
Carbon (C)
c)
Sulfur (S)
d)
Neon (Ne)
85.
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.
86.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
87.
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
88.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
89.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
90.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
91.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
92.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
93.
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
94.
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. 
95.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
96.
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.
97.
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
98.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
99.

Which type of element likes to give away electrons and become positive in a chemical reaction?

a)

metal

b)

nonmetal

c)

metalloid

100.

Which type of element likes to take electrons and become negative in a chemical reaction?

a)

metal

b)

nonmetal

c)

metalloid

101.

Every energy level (n) corresponds to a _________________ on the periodic table

a)

period

b)

group

c)

family

d)

block

102.

The majority of elements on the periodic table are:

a)

metals

b)

nonmetals

c)

metalloids

d)

synthetic

103.

ionization energy:

a)

Increases from left to right and increases down a group

b)

Decreases from left to right and increases down a group

c)

Decreases from left to right and decreases down a group

d)

Increases from left to right and decreases down a group

104.

Electronegativity:

a)

Increases from left to right and increases down a group

b)

Decreases from left to right and increases down a group

c)

Decreases from left to right and decreases down a group

d)

Increases from left to right and decreases down a group

105.

I am ready to SLAY this midterm

a)

Yes

b)

No

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