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U1P2 Exam Review

Total сұрақ: 64

Worksheet time: 1hrs 27mins

Аты
Сынып
Күн
1.

There may be a maximum of ____ p orbitals at a given energy level.

a)

2

b)

6

c)

3

d)

8

2.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

3.

Orbital sublevels, or L, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

4.

The proper pair of the L value with the orbital shape.

a)

0; f

b)

3; p

c)

1; s

d)

2; d

5.

With each higher energy level, the electrons are

a)

lower in energy

b)

more stable

c)

weaker

d)

farther from the nucleus

6.

How many electrons total are found in the f orbital?

a)

2

b)

6

c)

10

d)

14

7.

Which of the following is NOT a possible pair of quantum numbers?

a)

2p

b)

2d

c)

4p

d)

4f

8.

Which of the following sub levels correspond to n=3 l=2

a)

2p

b)

3s

c)

3p

d)

3d

e)

3f

9.

n=4, l=3?

a)

4f

b)

4d

c)

3s

d)

3p

10.

What is the maximum number of electrons that contain the values

n=4 l=3

a)

2

b)

6

c)

10

d)

14

e)

18

11.

Which of the following elements is Paramagnetic?

a)

Mg

b)

Ne

c)

P

d)

Ca

e)

Kr

12.

A paramagnetic atom is

a)

An atom with All paired electrons

b)

An atom with unpaired electrons

13.

An atom that is diamagnetic is

a)

An atom with all paired electrons

b)

An atom with unpaired electrons

14.

What is a possible set of quantum numbers of the last electron of Boron, 5B11.

a)

2,0,0,1/2

b)

2,0,0,-1/2

c)

2,1,2,1/2

d)

2,1,-1,1/2

15.

Which of the following set of quantum numbers is not valid?

a)

2,0,0,1/2

b)

2,0,1,1/2

c)

2,1,1,1/2

d)

2,1,0,1/2

16.

What is a possible set of quantum numbers of the electron 3s2?

a)

3,2,0,1/2

b)

3,0,0,-1/2

c)

3,1,1,1/2

d)

3,1,1,-1/2

17.

How many electrons can have the following set of quantum numbers, 6,0,0,1/2?

a)

1

b)

2

c)

3

d)

4

18.

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

a)

red

b)

black

c)

blue

d)

orange

19.

D block elements are known as .............

a)

Actinides

b)

Transition elements

c)

Lanthanides

d)

Noble gases

20.

What block is represented by the colour red?

a)

p-block

b)

d-block

c)

s-block

d)

f-block

21.

What block is represented by the colour blue?

a)

p-block

b)

d-block

c)

s-block

d)

f-block

22.

What block is represented by the colour yellow?

a)

p-block

b)

d-block

c)

s-block

d)

f-block

23.

What block is represented by the colour green?

a)

p-block

b)

d-block

c)

s-block

d)

f-block

24.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
25.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
26.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
27.
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.
28.
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
29.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
30.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
31.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
32.
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
33.
What is the Pauli Exclusion Principle?
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
34.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
35.
Which orbital shows a violation of the Aufbau Principle?
a)

1s2 3s2

b)

1s2 2s2

c)

1s2 2s2 2p6

d)

1s2 2s2 2p6 3s2

36.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
37.

What is the correct aufbau diagram for Nitrogen (N)?

a)
b)
c)
d)
38.

The correct electron configuration for Chlorine is

a)

1s22s22p5

b)

1s22s22p63s2

c)

1s22s22p63s23p4

d)

1s22s22p63s23p5

39.

The element Ca will form a cation. What would be the noble gas that this cation would have the same electron configuration as ?

a)

Ne

b)

Ar

c)

He

d)

Xe

40.

Which electron configuration belongs to a Chloride (Cl-) ion?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

d)

1s2 2s2 2p6 3p7

41.
What electron configuration matches an oxygen ion?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
42.

Write the electronic structure for Cr ion

a)
[Ar]4s13d5
b)
[Ar]4s13d2
c)
[Ar]4s03d3
d)
[Ar]3d3
43.
Write the electronic structure for Cu+1 ion
a)
[Ar]4s13d10
b)
[Ar]4s13d9
c)
[Ar]4s03d10
d)
[Ar]3d10
44.
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
45.

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 a bigger effective nuclear charge

d)

the atoms have less electrons.

46.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

47.

Which of these has the largest atomic radius?

a)

oxygen

b)

fluorine

c)

sulfur

d)

chlorine

48.

Order the following from smallest to largest atomic radius:

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

49.

The effective nuclear charge for a valence electron of magnesium is

a)

+1

b)

+2

c)

+12

d)

+24

50.

What is meant by isolectronic?

a)

Group of atoms or ions that have the same electronic configuration

b)

Group of atoms or ions that have the same protonic configuration

c)

Group of atoms or ions that have the same charges

d)

Group of atoms or ions that have different electronic configuration

51.

What is the example of species that are isolectronic species?

a)

Na+ and Mg2+

b)

Na+ and Na

c)

Na+ and Na2+

52.

Which species has the larger radius?

a)

Cl

b)

Cl-

53.

Which species has the larger radius?

a)

Na

b)

Na+

54.

Which is larger... P or P3- ? … and why?

a)

P3- because it gains an energy level

b)

P3- due to extra electron repulsion

c)

P because it loses an energy level

d)

P because of extra electron repulsion

55.

Arrange these species in increasing order of size.

Cl- , Ca2+ , S2- , Ar , K+

a)

Ca2+ > K+ > Ar > Cl- > S2-

b)

S2- > Cl- > Ar > K+ > Ca2+

c)

Ca2+ < K+ < Ar < Cl- < S2-

d)

S2- < Cl- < Ar < K+ < Ca2+

56.

Na+ and Al3+ are isoelectronic species (1s2 2s2 2p6). Which of these ion is smaller?

a)

Na+

b)

Al3+

c)

I'm not sure

d)

They have the same size

57.
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
58.

Ionization energy __________ as you do across a period

a)

has no pattern

b)

stays the same

c)

decreases

d)

increases

59.

Which has the highest ionization energy?

a)

Arsenic

b)

Iron

c)

ZInc

d)

Cobalt

60.
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
61.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
62.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
63.
Put these in order of increasing electronegativity:
Se, S, and O
a)
Se < S < O
b)
Se < O < S
c)
O < S < Se
d)
S < Se < O
64.
Chlorine and Fluorine are both very electronegative, as they are both missing a single electron from their valence energy level.  Why is Fluorine more electronegative than Chlorine? 
a)
Fluorine has less energy levels.
b)
Chlorine has more electrons in its outer shell
c)
Fluorine has more protons.
d)
None of these

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