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24-25 Chem Unit 2 Study Guide

Total questions: 121

Worksheet time: 2hrs 54mins

Name
Class
Date
1.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

2.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
3.
Measure mainly of the nuclear particles: protons + neutrons
a)
Subatomic Particles
b)
Atomic Number
c)
Atomic Mass
d)
Gluons
4.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
5.

Atoms of the same element with a different number of neutrons

a)

Ion

b)

alloy

c)

Isotope

d)

Quarks

6.
A charged atom
a)
Ion
b)
Isotope
c)
Electron Cloud
d)
Quark
7.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
8.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
9.
Arrangement of elements organized by atomic number
a)
Electron Cloud 
b)
Periodic Table 
c)
Electron Configuration
d)
None of these
10.

Calculation used to find the number of neutrons in an atom

a)

Mass Number- Atomic Number

b)

Atomic Number - Mass Number

c)

Mass Number - Electrons

d)

protons = electrons = neutrons

11.
How many protons does an aluminium atom have? (Use the image to help you)
a)
27
b)
14
c)
40
d)
13
12.
How many neutrons does a sodium atom have? (Use the image to help you)
a)
23
b)
11
c)
12
d)
34
13.
Atoms of the same element must always have the same number of _________
a)
electrons
b)
neutrons
c)
isotopes
d)
protons
14.
The _________ of an element equals the number of protons in an atom of that element
a)
mass number
b)
atomic weight
c)
atomic number
d)
isotopes
15.

The __________ of an atom is the sum of the protons and neutrons in the nucleus of that atom.

a)

mass number

b)

atomic number

c)

ionic charge

d)

isotope weight

16.

Which scientist was the first person responsible for proposing the idea of atoms?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

17.

Which scientist was the first person responsible for proposing the discovery of the electron?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

18.

Which scientist was the first person responsible for proposing the discovery of the nucleus?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

19.

Which scientist claimed that the atom was a small, dense, solid sphere?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

20.

Which scientist's model is referred to as the Plum Pudding Model?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

21.

Which scientist's model is referred to as the Planetary model?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

22.

Which scientist proposed the idea that the electrons orbited the nucleus on fixed paths with designated energies?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

23.

Which scientist proposed that the atom was indivisible using the word "atomos"?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

24.

Which scientist performed the Cathode Ray Experiment?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

25.

Which scientist performed the Gold Foil Experiment??

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

26.

Showed the atom was mostly empty space, and that the nucleus was small, dense, and positively charged.

a)

Rutherford

b)

Thomson

c)

Bohr

d)

Democritus

27.

The area of probability of finding an electron.

a)

Alpha

b)

Orbital

c)

Cathode

d)

Nucleus

28.
What can you conclude from the fact that scientists continue to update the atomic model?
a)
New information about atoms continues to be discovered
b)
Old information about atoms is completely useless
c)
Scientists did not have any information about atoms until a few years ago
d)
Scientists still have no idea what atoms look like
29.

Who discovered that the atom had an small, dense, positively charged center?

a)

Ernest Rutherford

b)

J.J Thomson

c)

Robert Millikan

d)

John Dalton

30.

Which scientist discovered that the atom has parts - which means it can be divided?

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

31.

In the atomic model nicknamed the "plum pudding" model, what do the plums represent?

a)

the nucleus

b)

the atom

c)

the electrons

d)

the positive material

32.

Different isotopes of an element contain different numbers of ___.

a)

protons

b)

neutrons

c)

electrons

d)

elements

33.

If a proton is added or removed from an atom, what happens?

a)

It becomes a different element.

b)

It becomes a different isotope.

c)

Nothing happens.

34.

How many neutrons are in 1 atom of Carbon-13?

a)

6

b)

13

c)

7

d)

20

35.

How many neutrons are in an atom of Nitrogen-16?

a)

9

b)

7

c)

16

d)

20

36.

How many protons are in an atom of Nitrogen-16?

a)

7

b)

9

c)

16

37.

What is the difference between Neon-20 and Neon-22?

a)

They have different numbers of electrons.

b)

They have different numbers of neutrons.

c)

Only 1 is radioactive.

d)

No difference.

38.

Which atom of these isotopes has 3 protons? The symbol for lithium is Li.

a)

Lithium-6

b)

Lithium-7

c)

All of them.

d)

Lithium-9

39.

How many neutrons are in this isotope?

a)

20

b)

41

c)

61

d)

21

40.

Which is the correct symbol for Fluorine-18?

a)
b)
c)
d)
41.

How many protons are in this isotope?

a)

9

b)

21

c)

12

42.

How would you write the isotope name from this nuclide symbol?

a)

Sodium-23

b)

Sodium-11

c)

Sodium-12

d)

Sodium-22

43.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
44.

These three isotopes of carbon have different -

a)

Atomic numbers

b)

Mass numbers

c)

Numbers of protons

d)

Symbols

45.

Which of these determines the identity of an atom?

a)

proton

b)

neutron

c)

valence electron

d)

protons and neutrons

46.

What is the correct hyphen notation name for the isotope with 19 electrons and 21 neutrons?

a)

Potassium-40

b)

Scandium-19

c)

Potassium-21

d)

Scandium-40

47.

What is the Atomic Number of Nitrogen?

a)

7

b)

14.007

c)

14

d)

21

48.

What is the Atomic Mass of Nitrogen?

a)

7

b)

14.007

c)

14

d)

21

49.

What is the Mass Number of Nitrogen?

a)

7

b)

14.007

c)

14

d)

21

50.

How many electrons are in an atom of Nitrogen?

a)

7

b)

14.007

c)

5

d)

2

51.

How many VALENCE electrons are in an atom of Nitrogen?

a)

7

b)

14.007

c)

5

d)

2

52.

How many energy levels of electrons are in an atom of Nitrogen?

a)

7

b)

14

c)

5

d)

2

53.

How many electrons are in the first energy level of an atom of Nitrogen?

a)

7

b)

14

c)

5

d)

2

54.

What period is Nitrogen in on the Periodic Table?

a)

7

b)

15

c)

5A

d)

2

55.

What group is Nitrogen in on the Periodic Table?

a)

7 (7B)

b)

15 (5A)

c)

5 (5B)

d)

2

56.

How many electrons will Nitrogen gain to fill its outer shell?

a)

2

b)

3

c)

5

d)

8

57.

What is the configuration for Carbon?

a)

1s2 2p2

b)

1s2 2s2 2p2

c)

1s1 1s2 2s2 2p2

58.

1s2 2s2 is which element?

a)

Lithium

b)

Beryllium

c)

Helium

d)

Boron

59.

Iron (Fe) configuration is

a)

1s2 2s2 2p6 3s2 3p3

b)

1s2 2s2 2p6 3s2 3p6 4s2

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d6

d)

1s2 2s2 2p6 3s2 3p6 4s2 4d6

60.

Which element is 1s2 2s2 2p6 3s2 3p6 4s2 3d7?

a)

Cobalt

b)

Nickel

c)

Manganese

d)

Chromium

61.

Write the configuration for Oxygen

a)

1s2 2s2 1p4

b)

2s2 2p4

c)

1s2 2s2 3p4

d)

1s2 2s2 2p4

62.

Write the configuration for Phosphorus

a)

2s2 2p6 3s2 3p3

b)

1s2 2s3 2p6 3p3

c)

1s2 2s2 2p6 3s2 3p3

d)

1s2 2s2 2p5 3s2 3p3

63.

Which element is 1s2 2s2 2p6 3s2 3p6 4s1?

a)

Sodium (Na)

b)

Lithium (Li)

c)

Potassium (K)

d)

Calcium (Ca)

64.

Choose the correct configuration for Zinc

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d9

c)

1s2 2s2 2p6 3s2 3p6 3s2 3d10

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

65.

Choose the correct element for 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

a)

Chlorine

b)

Bromine

c)

Krypton

d)

Sulfur

66.

Choose the correct configuration for Neon (Ne).

a)

1s2 2s2 2p6 3s2 3p6

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6

d)

1s2 2s1 2p6

67.
The type of spectrum generated here is called...
a)
absoption
b)
continuous
c)
constant
d)
emission
68.
Light is emitted when electrons ...
a)
jump from high to low 
b)
jump from low to high 
c)
either of these
d)
none of these
69.

The color of emitted light with the LONGEST wavelength is

a)

violet

b)

green

c)

red

d)

indigo

70.

The color of emitted light with the greatest energy per photon is:

a)

violet

b)

green

c)

red

d)

indigo

71.

The color of emitted light with the HIGHEST frequency is

a)

violet

b)

green

c)

red

d)

indigo

72.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Helium

73.
How many sublevels are contained in the n=3 principal energy level?
a)
1
b)
2
c)
3
d)
6
74.
Emission lines create _____ spectral lines on a visible light spectra due to the electrons moving into their _____ state.
a)
dark; excited
b)
dark; ground
c)
bright; excited
d)
bright; ground
75.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
76.
All electromagnetic waves have the same...
a)
frequency
b)
speed
c)
wavelength
d)
energy
77.
What is the number of wave cycles that pass a given point per unit of time
a)
crest
b)
wavelength
c)
frequency
d)
amplitude
78.
The equation that shows the relationship between the energy of light and frequency is: 
a)
c= λ⋅f
b)
E=h⋅f
79.
Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 × 10 10 1/s.
a)
6.63 x 10-34 J
b)
5.25 x 1014 J
c)
5.24 x 10-23 J
d)
1.19 x 1044 J
80.

Red light has a wavelength of 675 x 10-9 m. What is its frequency?

a)

2.03x1011 m

b)

4.44x1014 Hz

c)

4.44x1014 nm

d)

2.03x1011 Hz

81.

What is the speed of light?

a)

3.0x108 ms

b)

3.0x108 m/s

c)

6.626x10-34 Js

d)

6.626x10-34 J/s

82.

Ground state means that an electron is...

a)

at its lowest possible potential energy

b)

in the first shell of an atom

c)

laying low for the weekend

d)

removed from an atom

83.

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

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

84.
Which type of orbital is shaped like a sphere?
a)
s orbital
b)
p orbital
c)
d orbital
d)
f orbital
85.

What does the 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

86.

How many total electrons can can 5 d orbitals hold?

a)

14

b)

10

c)

2

d)

6

87.

What are the orbitals for n=4

a)

s

b)

s, p

c)

s, p, d

d)

s, p, d, f

88.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

89.
Which of the following statements is true about the 3s and the 4s sublevels?
a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
90.

What would this atom want to do to become stable

a)

Gain 3 electrons to get a +3 charge

b)

Gain 5 electrons to get a +5 charge

c)

Gain 3 electrons to get a -3 charge

d)

Gain 5 electrons to get a -5 charge

91.

Which of the following describes electrons in the modern periodic table?

a)

Floating motionless in space

b)

In energy levels orbiting the nucleus like planets around the sun

c)

In energy levels, moving as both particles and waves in areas of 90% probability called orbitals

d)

Moving totally at random in the electron cloud.

92.
Coulombic Attraction is the attraction between __________ charged particles.
a)
same 
b)
oppositely
c)
two positively
d)
two negatively
93.
An example of Coulombic Attraction in an atom is between
a)
protons and neutrons
b)
neutrons and electrons
c)
protons and electrons
d)
protons and protons
94.
As the distance between protons and electrons increases, the force of attraction
a)
remains the same
b)
increases
c)
decreases
d)
is not affected
95.
If distance remains the same, as the number of protons increases, the force of attraction
a)
remains the same
b)
increases
c)
decreases
d)
is divided by 1/2
96.
What are the two variables that affect Coulombic Attraction?
a)
Distance  and number of protons
b)
Number of neutrons and number of protons
c)
Number of neutrons and number of electrons
d)
solids or liquids
97.

Looking at atoms in the same group/family (column), what factor most greatly affects Coulombic attraction?

a)

number of protons

b)

distance from the nucleus

c)

moles of atoms

d)

number of neutrons

98.

What is the trend in Coulombic attraction going down a group?

a)

Coulombic attraction increases moving down a group.

b)

Coulombic attraction decreases moving down a group.

99.

What is the trend in Coulombic attraction moving from left to right across a period?

a)

Coulombic attraction increases moving from left to right across a period.

b)

Coulombic attraction decreases moving from left to right across a period.

100.

Select the element that has the strongest Coulombic attraction.

a)

O

b)

S

c)

Se

d)

Te

101.

Select the element that has the strongest Coulombic attraction.

a)

O

b)

F

c)

N

d)

C

102.

Select the element that has the strongest Coulombic attraction.

a)

Fe

b)

Mn

c)

Zn

d)

Sc

103.

Select the element that has the strongest Coulombic attraction.

a)

Li

b)

Na

c)

Rb

d)

Cs

104.

What are the two variables that affect Coulombic Attraction?

a)

Distance and number of protons

b)

Number of neutrons and number of protons

c)

Number of neutrons and number of electrons

d)

Distance and number of neutrons

105.

What is the trend in Coulombic attraction moving from left to right across a period?

a)

Coulombic attraction increases moving from left to right across a period.

b)

Coulombic attraction decreases moving from left to right across a period.

c)

No trend can be observed.

d)

The trend depends upon which period is being observed.

106.

What is the trend in Coulombic attraction going down a group?

a)

Coulombic attraction increases moving down a group.

b)

Coulombic attraction decreases moving down a group.

c)

No trend can be observed.

d)

The trend depends upon which group is being observed.

107.

Which of the following will have similar properties?

a)

O, S, Se

b)

O, F, Ne

c)

N, Ne, Na

d)

H, K, P

108.
Each column in the periodic table is called a _________ .
a)
period
b)
group
c)
cluster
d)
unit
109.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
110.

How many periods are on the periodic table?

a)

5

b)

6

c)

7

d)

8

111.

Elements in the same group have : (2 correct answers)

a)

Similar chemical properties

b)

Similar names

c)

Same number of outer (valence) electrons)

d)

The same number of protons

112.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
113.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
114.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
115.

Match the following elements to the group they belong to.

a)

sodium

1.

alkali metal

b)

calcium

2.

alkaline earth metal

c)

chlorine

3.

halogen

d)

argon

4.

noble gas

116.

The PES spectrum below is for the element _______________.

a)

O

b)

Ne

c)

N

d)

F

117.

Examine the spectrum below. Where would you expect the 2p peak for F be if it were on the same spectrum?

a)

To the left of the peak at 3.04

b)

To the right of the peak at 3.04

c)

To the left of the peak at 1.31

d)

To the right of the peak at 1.31

118.

Which peak (or peaks) correspond to the valence electrons?

a)

The peak at 1

b)

The peaks at 1 and 2.05

c)

The peak at 239

d)

The peaks at 239 and 22.7

119.

What is the electron configuration for this PES graph?

a)

1s22s22p63s23p2

b)

1s22s22p63s23p1

c)

1s22s22p63s23p3

d)

1s22s22p63s2

120.

Which element is represented by this PES graph?

a)

argon

b)

potassium

c)

calcium

d)

scandium

121.

Which electrons should have the greatest binding energy?

a)

Electrons closest to the nucleus

b)

Electrons that are in the valence shell

c)

Electrons that experience the most electron shielding

d)

All electrons experience equivalent binding energy

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