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Unit 2 HCHEM Atomic structure review

Total questions: 65

Worksheet time: 2hrs 30mins

Name
Class
Date
1.

Rutherford's gold foil experiment provided evidence for which of the following statements?

a)

Negative and positive charges are spread evenly throughout an atom.

b)

Alpha particles have a positive charge.

c)

Gold is not as dense as previously thought.

d)

There is a dense, positively charged mass in the center of an atom.

2.

In an atomic model that includes a nucleus, positive charge is

a)

concentrated in the center of an atom

b)

spread evenly throughout an atom.

c)

concentrated at multiple sites in an atom

d)

located in the space outside the nucleus

3.

Which statement about subatomic particles is true?

a)

Protons, neutrons, and electrons all have about the same mass.

b)

Unlike protons or neutrons, electrons have no mass.

c)

Neutrons have no charge and no mass.

d)

An electron has far less mass than either a proton or neutron.

4.

Which of the following is unique for any given element?

a)

the number of neutrons

b)

the charge on the electrons

c)

the number of protons

d)

the mass of a neutron

5.

The number of protons in one atom of an element is that element's

a)

mass number.

b)

balanced charge.

c)

atomic number.

d)

isotope.

6.

How would you find the number of neutrons in a an atom?

a)

atomic number - mass number

b)

mass number - atomic number

c)

electron number - atomic number

d)

atomic number - isotope number

7.

Which statement is true about oxygen-17 and oxygen-18?

a)

They do not have the same number of protons.

b)

Their atoms have an identical mass.

c)

They are isotopes of oxygen.

d)

They have the same mass number.

8.

Which statement accurately represents the arrangement of electrons in the Bohr's atomic model?

a)

Electrons vibrate in fixed locations around the nucleus.

b)

Electrons travel around the nucleus in fixed energy levels with energies that vary from level to level.

c)

Electrons travel randomly in the relatively large space outside the nucleus.

9.

What is the difference between an atom in the ground state and an atom in an excited state?

a)

The atom in the ground state has less energy and is less stable than the atom in an excited state.

b)

The atom in an excited state has one fewer electron than the atom in the ground state.

c)

The atom in an excited state has more energy and is less stable than the atom in the ground state.

d)

The atom in an excited state has one more electron that the atom in the ground state.

10.

In Rutherford's gold foil eperiment, alpha particles bounce straight back from the foil having struck __________ in the gold atoms.

a)

nulcei

b)

electrons

c)

empty space

d)

gold

11.

Protons and ________ are found in the nucleus of an atom.

a)

hydrogen

b)

atoms

c)

electrons

d)

neutrons

12.

If element "A" has 23 protons, its ______________________ is (are) 23.

a)

electrons

b)

mass number

c)

atomic number

d)

neutrons

13.

The nuclei of isotopes contain different numbers of ________.

a)

protons

b)

neutrons

c)

electrons

d)

atomic numbers

14.

The region in which an electron is most likely to be found is called a(an) ________________.

a)

atom

b)

electron spot

c)

orbital

d)

nucleus

15.

An atom in which an electron has moved to a higher energy level is in a (an) ______ state.

a)

excited

b)

ground

c)

neutral

d)

positive

16.

What is 8?

a)

atomic number

b)

mass number

c)

atomic weight

d)

isotope

17.

O is the

a)

atomic number

b)

atomic symbol

c)

atomic name

d)

atomic weight

18.

Oxygen is the atomic

a)

number

b)

weight

c)

symbol

d)

name

19.

15.999 is the atomic

a)

weight

b)

number

c)

electron

d)

name

20.

What is the mass number Beryllium if you have 5 neutrons?

a)

10

b)

8

c)

9

d)

11

21.

What is the isotope symbol of nitrogen if it has 7 neutrons?

a)

nitrogen-14

b)

nitrogen-7

c)

nitrogen-8

d)

nitrogen-15

22.

What is the element symbol if the atomic number is 15?

a)

N

b)

O

c)

S

d)

P

23.

How many neutrons does boron-11 have?

a)

5

b)

6

c)

7

d)

11

24.

If the:

Atomic number = 15

Mass number = 31


How many electrons do you have?

a)

15

b)

16

c)

30

d)

31

25.

In a Bohr Diagram, how many electrons will go in each shell?

a)

2, 6, 16

b)

2, 6, 18

c)

2, 4, 6

d)

2, 8, 18

26.

In the Bohr diagram for the element Aluminum, how many electrons will go in each shell?

a)

2, 8, 3

b)

2, 8, 18

c)

3, 8, 2

d)

2, 6, 5

27.

Which particles change the charge in atoms when ions are formed?

a)

Protons

b)

Electrons

c)

Neutrons

28.

Cations are...

a)

Positive

b)

Negative

c)

Neutral

29.

Anions are...

a)

Positive

b)

Negative

c)

Neutral

30.

An atom becomes _________ when it gains electrons.

a)

Positive

b)

Negative

c)

Neutral

31.

An atom becomes _______ when it loses electrons.

a)

Positive

b)

Negative

c)

Neutral

32.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
33.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
34.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
35.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
36.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
37.
Isotopes are atoms of the same element with different #’s of __________ & therefore different __________.
a)
n0 ;  atomic #’s
b)
p+ ; atomic #’s
c)
e- ; atomic masses
d)
n0 ; atomic masses
38.
An atom is electrically neutral when
a)
protons and neutrons are the same
b)
protons and electrons are the same
c)
neutrons and electrons are the same
d)
neutrons balance the protons and electrons
39.
Two isotopes of carbon are carbon-12 and carbon-14.  These isotopes differ from one another by two protons.
a)
true
b)
false
40.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
41.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
42.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
43.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
44.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
45.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
46.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
47.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
48.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
49.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
50.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
51.
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 there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
52.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
53.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
54.

What are the four energy sublevels?

a)

s, p, d, and f

b)

a, b, c, and d

c)

w, x, y, and z

d)

1, 2, 3, and 4

55.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

56.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

57.

Which of the following is the orbital notation for oxygen?

a)
b)
c)
d)
58.
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.
59.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
60.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
61.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
62.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
63.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?  
I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
64.

An unknown element has three isotopes. Given the abundances and relative masses, determine (from the periodic table) which element it is.

Abundances | Relative masses

0.005% | 234.04 amu

0.720% | 235.04 amu

99.275% | 238.05 amu

HINT: You do NOT need to calculate anything here.

a)

Uranium (#92, Atomic Mass: 238.03 amu)

b)

Fluorine (#9, Atomic Mass: 19.00 amu)

c)

Mercury (#89, Atomic Mass: 200.59 amu)

d)

Polonium (#84 209 amu)

65.

Element Z has 2 natural isotopes. One isotope has a mass of 15.0 amu and a relative abundance of 30%. The other isotope has a mass of 16.0 amu and a relative abundance of 70%. Estimate the average atomic mass for this one element.

a)

15.0 amu

b)

16.0 amu

c)

15.7 amu

d)

16.9 amu

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