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Unit 2 Particles

Total questions: 88

Worksheet time: 2hrs 35mins

Name
Class
Date
1.

Who was the first person to "think" of an atom?

a)

Democritus

b)

J.J. Thompson

c)

Rutherford

d)

Bohr

2.

Which one of these is Dalton's Model?

a)
b)
c)
d)
3.
Matter always has mass.
a)
true
b)
false
4.

What is a particle with one positive charge called?

a)

proton

b)

electron

c)

neutron

d)

quark

5.

Which model was created after the discovery of the electron cloud?

a)

Dalton's

b)

Rutherford's

c)

Quantum Mechanical

d)

Plum Pudding

6.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

7.

Look at this picture of Argon off the periodic table. Which of the following is true for this element?

a)

18 protons

b)

40 protons

c)

22 protons

d)

21.9 protons

8.
The nucleus of an atom is made of
a)
electrons and protons
b)
electrons and neutrons
c)
protons and neutrons
d)
empty space
9.
If an atom contains exactly three protons, then it's an atom of _____
a)
lithium
b)
gold
c)
nitrogen
d)
carbon
10.
For an atom to be electrically neutral, it must contain the same number of _____
a)
protons and neutrons
b)
neutrons and electrons
c)
protons and electrons
d)
nucleons and electrons
11.
The middle of the atom, which contains protons and neutrons, is called _____
a)
the shell
b)
the nucleus
c)
the cell
d)
the control center
12.

Which part of an atom has the smallest mass?

a)

Proton

b)

Neutron

c)

Electron

d)

They are all the same

13.

Using the picture from a periodic table, what is the Atomic Number?

a)

26

b)

Fe

c)

55.845

d)

56

14.

Using the picture from a periodic table, what is the Atomic Mass?

a)

26

b)

Fe

c)

55.845

d)

56

15.

Using the picture from a periodic table, what is the Mass Number?

a)

26

b)

Fe

c)

55.845

d)

56

16.

Using the picture from a periodic table, how many PROTONS are in Iron?

a)

26

b)

30

c)

55.845

d)

56

17.

Using the picture from a periodic table, how many NEUTRONS are in Iron?

a)

26

b)

30

c)

55.845

d)

56

18.

When two atoms of the same element have different masses, they are called ______, and have a different number of ______.

a)

Neutrons; Isotopes

b)

Atoms; Isotopes

c)

Isotopes; Protons

d)

Isotopes; Neutrons

19.

Which of the following atoms is an isotope?

a)

C-14

b)

S2-

c)

Al3+

d)

He

20.

What charge does an atom have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

21.

What is a representation of an ion?

a)

Li

b)

Na-22

c)

O-2

22.
A neutral atom would become an ion that has a charge of 2+ by 
a)
Losing two protons
b)
Losing two neutrons
c)
Losing two electrons
23.
Isotopes are atoms that have different
a)
Mass numbers
b)
Element names
c)
Atomic Numbers
24.

Using the atomic masses and relative abundance of the isotopes of nitrogen given below, determine the average atomic mass of nitrogen.

N-14: 14.003 amu; 99.63% N-15: 15.000 amu; 0.37%

a)

14.003 amu

b)

14.007 amu

c)

14.506 amu

d)

15.000 amu

25.

An archaeologist discovers an ancient wooden bowl. Which isotope would most likely be used to determine its age?

a)

carbon–12

b)

carbon–14

c)

uranium–238

d)

oxygen-16

26.
How are electrons arranged in an atom?
a)
In groups of five
b)
In energy levels
c)
By color
d)
By shape
27.

According to Bohr, what two things do electrons have to have enough energy to do?

a)

Resist the energy given to it by a photon

b)

Stay in constant motion around its orbital

c)

Resist the attraction from the positive nucleus

d)

Jump between energy levels

28.

The subshells are represented by the possible letters: s, p, d, or f.

a)

True

b)

False

29.

The ground state is when an electron in an atom is excited into the lowest possible vacant orbita

a)

True

b)

False

30.

Which subshell letter corresponds to a spherical orbital?

a)

s

b)

p

c)

d

d)

f

e)

not enough information

31.

Which statement is true about "p" orbitals?

a)

A subshell that contains three "p" orbitals.

b)

These orbitals are shaped like dumbbells.

c)

A 3p orbital has a higher energy than a 2p orbital.

d)

All of these statements are true

32.

The "d" subshell can hold a maximum of ________ electrons.

a)

2

b)

5

c)

6

d)

10

e)

14

33.

The subshell that has three orbitals and can hold up to six electrons is the:

a)

s subshell

b)

p subshell

c)

d subshell

d)

f subshell

34.

The probability map for an electron is called

a)

an orbit

b)

a photon

c)

an orbital

d)

an electron configuration

35.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
36.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
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.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
39.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
40.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

41.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

42.

Which of the following is the orbital notation for oxygen?

a)
b)
c)
d)
43.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
44.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
45.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
46.
What is the correct noble-gas notation for the electron configuration of an atom of chlorine? 
a)
a. [Ar]3s2 3p5
b)
 b. [Ne]3s2 3p4
c)
 c. [Ar]3s2 3p4
d)
 d. [Ne]3s2 3p5
47.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

location on the table.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

48.

What subatomic particle is responsible for the spectral lines seen in emission spectra diagrams?

a)

electrons

b)

protons

c)

neutrons

49.

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

a)

emit energy

b)

absorb energy

c)

wiggle

50.

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

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

51.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
52.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

53.

In which state does an electron have the least amount of energy?

a)

Excited state

b)

Ground state

c)

Orbital

d)

Bohr model

54.
Line emission spectrum shown below happens when
a)
Electron transition from lower to higher energy level.
b)
Electron transition from higher to lower energy level.
c)
Electron exist in fixed energy states
d)
Electron transition between different energy levels.
55.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
56.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

location on the table.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

57.

The ground state is the ______________ energy state of an atom.

a)

highest

b)

lowest

58.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
59.
Which has the LONGEST wavelength and, therefore, the lowest frequency/energy
a)
Gamma Rays
b)
Radio Waves
c)
Visible Light
d)
Infrared rays
60.
Which has the SHORTEST wavelength and, therefore, the highest frequency/most energy
a)
Radio waves
b)
Ultraviolet Rays
c)
Gamma Rays
d)
X-rays
61.
Which section of the spectrum is the ONLY one we can see?
a)
X-rays
b)
Visible Light
c)
Gamma Rays
d)
Ultraviolet Rays
62.
The height of the wave is known as the _____________.
a)
amplitude
b)
crest
c)
trough
d)
wavelength
63.
The blue section of the wave is measuring _________________.
a)
wavelength
b)
crest
c)
trough
d)
amplitude 
64.
Light behaves like both a particle and a ______.
a)
Mass
b)
Wave
c)
Current
65.
High frequency waves have _________ wavelengths.
a)
varying
b)
long
c)
the same
d)
short
66.
The relationship between wavelength and frequency is λ=c/f.  Calculate the wavelength of light that has a frequency of 5.2 x 1012 1/s. The speed of of light is 3.0x 108 m/s.
a)
5.8 x 10 -5 m
b)
5.8 x 10 -7 m
c)
5.19 x 10 14 m
d)
1.56 x 10 23 m
67.
Solve this problems using the equation: 
C = λν
If an AM radio station broadcasts at
9.95 x 105 Hz, what is the wavelength of this radiation?
a)
6.59 x 10-28 m
b)
1.01 x 10-6 m
c)
3.32 x 10-3 m
d)
302 m
68.

IRAS, the Infrared Astronomy Satellite launched by NASA in 1983, had a detector that measured infrared or heat radiation from different regions of space. What is the frequency of infrared light that has a wavelength of

1.10 X 10-6 m?

a)

3.67 x 10-15 Hz

b)

3.67 x 10-3 Hz

c)

2.73 x 102 Hz

d)

2.73 x 1014 Hz

69.

A common infrared laser operates at 1.06 x 103 nm. What is the energy of a photon with this wavelength? (1 x 109 nm = 1m)

a)

7.02 x 10^-40 J

b)

6.25 x 10^-28 J

c)

3.54 x 10^-15 J

d)

1.87 x 10^-19 J

70.
Who arranged the first periodic table.
a)
Mosely
b)
Einstein
c)
Mendeleev
d)
Bohr
71.
Mendeleev classified elements based on not only atomic mass but what else?                                                   
a)
reactivity
b)
boiling points
c)
physical properties only 
d)
 chemical & physical properties
72.
Why were there blank spaces left in Mendeleev's periodic table?                                              
a)
He didn't know what to put there.
b)
 Undiscovered elements not yet known.
c)
Multiple elements could have fit
d)
He forgot to add the elements in.
73.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
74.

what is the big group of metals called found within the metals

a)

transition metals

b)

nonmetals

c)

noble gases

d)

halogens

75.
Atoms with similar properties are most likely located...
a)
in the same period.
b)
in the same group.
c)
in different periods.
d)
to the right and left of each other.
76.

Which element is most likely to have six electrons in its 4th energy level?

a)

Oxygen (O)

b)

Selenium (Se)

c)

Krypton (Kr)

d)

Potassium (K)

77.

Which color on the image of the periodic table corresponds with the actinides.

a)

red

b)

black

c)

blue

d)

yellow on bottom

78.

Part of the Periodic Table is shown.

The letters are not the symbols of the elements.

Which element is a non-metal?

a)

A

b)

B

c)

C

d)

D

79.

Which statement describes noble gases?

a)

They all have eight electrons in their outer shell.

b)

They are monatomic gases.

c)

They form ions with full outer shells of electrons.

d)

They react with oxygen to form unreactive compounds.

80.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
81.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
82.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
83.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

84.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

85.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

86.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

87.

What is one-half the distance between the nuclei of identical atoms that are bonded together?

a)

atomic radius

b)

atomic diameter

c)

atomic width

d)

atomic length

88.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

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