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Electron Config and Periodicty

Total questions: 80

Worksheet time: 2hrs 46mins

Name
Class
Date
1.
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
2.
An argon ion laser emits light at 488 nm. What is the frequency of this radiation? (1 nm = 1x10-9m)
a)
4.07 x 10-19 Hz
b)
6.15 x 1014 Hz
c)
1.46 x 102 Hz
d)
2.05 x 106 Hz
3.
What is the frequency of a photon whose energy is 3.4x10-19J?
a)
8.8x1026 Hz
b)
5.1x1014 Hz
c)
1.9x10-15 Hz
d)
2.3x10-52 Hz
4.
Which of the following regions of the electromagnetic spectrum has the longest wavelengths?
a)
microwave
b)
infrared
c)
x-ray
d)
gamma ray
5.
Which of the following regions of the electromagnetic spectrum has the lowest frequency?
a)
ultraviolet
b)
infrared
c)
visible
d)
x-ray
6.
An radium-266 atom may emit a photon of light with a frequency of 4.50 x 1019 Hz when it undergoes nuclear fission. What is the wavelength (in pm) of this photon?
a)
0.0298 pm
b)
6.66 pm
c)
15.0 pm
d)
29.8 pm
7.
As an electron moves from n=1 to n=4, is energy absorbed or released?
a)
Absorbed
b)
Released
8.
As an electron moves from n=4 to n=1, is energy absorbed or released?
a)
absorbed
b)
released
9.
What type of radiation has the lowest energy and highest energy, respectively?
a)
Radio - Gamma
b)
Gamma - Radio
c)
Visible - Infrared
d)
Infrared - Visible
10.
A common infrared laser operates at 1.06 x 103 nm. What is the energy of a photon with this wavelength? (1 nm = 1x10-9m)
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
11.
The maximum number of electrons that can be placed in an p orbital.  
a)
2
b)
6
c)
10
d)
14
12.

How many unpaired electrons are in Cr+3?

a)

0

b)

1

c)

2

d)

3

13.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
14.

Which of the following is true?

a)

An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins

b)

An atomic orbital can hold a minimum of 6 electrons, each with opposite spins

c)

An atomic orbital can hold a maximum of 6 electrons, each with the same spin

d)

An atomic orbital can hold a minimum of 2 electrons, each with opposite spins

15.
What orbital is shown in the picture?
a)
s
b)
p
c)
d
d)
f
16.

write the abbreviated electron config for Strontium?

a)

[Kr] 3s2

b)

[Kr] 4s2

c)

[Kr] 5s2

d)

[Ar] 5s2

17.

Which orbital is displayed correctly?

a)

A

b)

B

c)

C

d)

D

18.

The electron configuration of an atom is 1s22s22p63s23p2 The number of valence electrons in the atom is

a)

2

b)

4

c)

8

d)

10

19.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
20.

How many electrons can an f sublevel hold?

a)

2

b)

6

c)

10

d)

14

21.

How many valence electrons does aluminum?

a)

13

b)

1

c)

3

d)

5

22.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
23.

What electron configuration matches the ion: Al +3

a)

1s22s22p63s23p4

b)

1s22s22p6

c)

1s22s22p63s23p1

d)

1s22s22p63s2

24.
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.
25.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
26.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
27.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
28.
The impossibility to know simultaneously the exact position and momentum of a particle is called the:
a)
Einstein Uncertainty Principle
b)
Moseley Uncertainty Principle
c)
Heisenburg Uncertainty Principle
d)
Bohr Uncertainty Principle
29.

The 3rd energy level can hold up to ___ electrons

a)

8

b)

18

c)

14

d)

16

30.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
31.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
32.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
33.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
34.
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)
There should only be 1 arrow in the first 2p box and one arrow in the 2nd 2p box both pointing up
d)
All the arrows should be pointing up.
35.

Which of the following is the ground state electron configuration of Ni?

a)

1s22s23s23p64s23d6

b)

1s22s22p63s23p64s23d8

c)

1s22s22p63s23p64d8

d)

1s22s23s23p64s33d6

36.

The element that has a valence configuration (outermost electrons) of 5s2 is

a)

Ba

b)

Sr

c)

Rf

d)

Y

37.

The ground-state electron configuration of the element ________________ is [Kr] 5s24d7.

a)

Rh

b)

Ir

c)

Co

d)

Cd

38.
How many unpaired electrons would lithium have?
a)
1
b)
2
c)
3
d)
0
39.
What is the electron configuration of Ag?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10
b)
[Kr] 5s2 4d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d9
d)
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4d10 4p6 5d10 5s2 4d9
40.

Which electron configuration belongs to Copper (Cu)?

a)

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

b)

1s2 2s2 2p6 3s2 3p6 4s1 3d10

c)

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

41.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
42.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings 
43.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
44.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
45.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
46.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
47.
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
48.
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.
49.
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
50.
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.
51.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
52.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

53.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
54.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
55.
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 
56.
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
57.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
58.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
59.
Choose the set that goes from lowest to highest electronegativity?
a)
Cu, Mg, Sr, Ca
b)
F, Cl, Br, Si
c)
Cs, Rb, Ca, Mg
d)
Zn, Cd, Ag, Cu
60.

Which lists of 4 elements correctly aligns them left to right in order of decreasing atomic radius?

a)

O > P > K > Mg

b)

K > Mg > P > O

c)

Mg > K > P > O

61.
Which of the following atoms has the lowest electronegativity?
a)
Cs
b)
Cl
c)
C
d)
Cu
62.

Which is correct representation of an Ca atom or Ca cation?

a)

atom is smaller than a cation

b)

cation is smaller than original atom

c)

atom and cations always are positive charged

63.

Which is a true statement?

a)

Anions are always the smallest and negatively charged

b)

Anions are the same size as the original atom; same charge

c)

Anions are bigger from the atom from which they come ; negatively charge

d)

Anions are smallest and positively charged

64.
Of the following ions has the largest ionic radius
a)
Ca+
b)
Sr+
c)
Sc+
d)
Y+
65.
What is the most likely ion that Ca will form
a)
Ca +
b)
Ca -
c)
Ca 2+
d)
Ca 2-
66.
What is the most likely ion that Cl will form
a)
Cl +
b)
Cl -
c)
Cl 2+
d)
Cl 2-
67.

Which has the greatest 2nd ionization energy:

a)

Ca

b)

K

c)

Al

d)

Se

68.
the electronic configuration for an oxygen ion is
a)
1s2 2s2 2p4
b)
1s2 2s2 2p6
c)
1s2 2s2 2p6 3s2 3p4 
d)
1s2 2s2 2p6 3s2 3p6
69.
The early periodic table organized the elements in periods of increasing atomic mass. What information is currently used to organize the elements on the periodic table?
a)
number of valence electrons 
b)
number of energy levels 
c)
atomic number 
d)
ionic radius 
70.
The number of valence electrons in an element affects the reactivity of that element. Which element listed has the fewest valence electrons?
a)
beryllium (Be)
b)
sodium (Na) 
c)
oxygen (O) 
d)
neon (Ne)
71.
What is the family name of this group of elements? 
a)
Alkali metals 
b)
Halogens 
c)
Noble Gases 
d)
Alkali Earth Metals 
72.
Using the Periodic Table of the Elements, the properties of elements can often be used to deduce the properties of neighboring elements. In which set can the reactivity of the first three elements be used to most accurately predict the reactivity of the fourth element?
a)
silver (Ag), sodium (Na), strontium (Sr) → sulfur (S)
b)
fluorine (F), oxygen (O), nitrogen (N) → carbon (C)
c)
antimony (Sb), tellurium (Te), iodine (I) → xenon (Xe)
d)
oxygen (O), sulfur (S), tellurium (Te) → selenium (Se)
73.
The ionization potential of an element is the amount of energy required to remove an electron from an isolated atom or molecule. According to the periodic table, which of the following indicates the correct decreasing order of ionization energy?
a)
Li > Na > K > Cs
b)
Na > K > Li > Cs
c)
Li > K > Na > Cs 
d)
Cs > K > Na > Li 
74.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
75.
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
76.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
77.

Which is the largest ion?

a)

P3-

b)

S2-

c)

Ca2+

d)

Cl-

78.

Which order is correct when the size of atoms and ions are compared?

a)

O2- > O-

b)

Cl > Br

c)

Cl+ > Cl

d)

K+ > K

79.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

80.
Valence Electrons determine an element's _____________.
a)
Reactivity
b)
Location
c)
Identity
d)
Color

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