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E1S2 Quiz 2 - Chapter 2 : Electronic Structure of Atom

Total questions: 40

Worksheet time: 29mins

Name
Class
Date
1.

Read and choose the correct following statements :


I. The dense protonic nucleus is surrounded of electrons.

II. Electrons are revolving in concentric orbits

III. Energies of the electrons are quantized

a)

I and II

b)

II and III

c)

I and III

d)

I, II and III

2.

One of the uses of the emission line spectrum of a specific substance is to:

a)

Identify unknown substances

b)

Obtain the electromagnetic spectrum

c)

Know the energy level of the electrons

d)

Know the position of the electrons

3.

Which of the following electron transition occurs in the ultraviolet range of the electromagnet spectrum?

a)

n3 to n1

b)

n3 to n2

c)

n4 to n3

d)

n2 to n3

4.

The emission spectrum of hydrogen atom is a line spectrum because

a)

energy is required to excite an electron

b)

electrons which are unstable will radiate energy

c)

an excited electron has a higher energy and is not stable

d)

the energy of an electron an a hydrogen atom is quantised

5.

One of the lines in the spectrum of hydrogen atom has a frequency of 7.80 x 1014 s-1. What is the wavelength of this line? (c = 3 x 108 ms-1)

a)

2.34 x 1014 m

b)

2.34 x 1013 m

c)

3.85 x 10-7 m

d)

3.84 x 1013

6.

An excited electron residing in the energy level n = 4 drops to n = 1. What is the wavelength of the emission if the frequency is 3.09 x 1015 Hz? (c = 3 x 108 ms-1)

a)

4.69 x 10-6 m

b)

2.91 x 10-7 m

c)

3.88 x 10-7 m

d)

9.71 x 10-8 m

7.

Which of the following statements regarding the hydrogen atom spectrum is not correct

a)

The single electron in hydrogen jumps to higher energy levels.

b)

The energy of an electron in a hydrogen atom is quantised.

c)

Hydrogen is the only element that can produce an atomic spectrum.

d)

When an electron has the smallest allowable amount of energy, it is in the ground state.

8.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
9.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
10.
The electron configuration of an atom is 1s22s22p6.  The number of valence electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
11.

What electron configuration matches an oxygen ion? (Z=8)

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

12.

Write the electronic configuration for sodium Na (Z=11)

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s1

d)

1s2 2s2 2p6 3s2 3p4

13.

State the valence electronic configuration for Mg (Z=12)

a)

3s2

b)

3s2 3p1

c)

3s2 3p3

d)

3s2 3p4

14.

Determine the element that has valence electron 3s23p1

(Z of Na = 11, Al = 13, Cl = 17, Mg = 12)

a)

Na

b)

Al

c)

Cl

d)

Mg

15.

Electron must be arrange from lowest energy to highest energy.

State the rule/principle?

a)

Hund's Rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

Zuhaizi Principle

16.

Which element is pictured?

a)

neon (Z=10)

b)

fluorine (Z=9)

c)

magnesium (Z=12)

d)

argon (Z=18)

17.

All ions matches with this electronic configuration.Except?

1s22s22p63s23p6

a)

Al3+

b)

Cl-

c)

S2-

d)

Ca2+

18.

What electron configuration matches an oxygen atom?

(Z = 8)

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

19.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
20.

In 1s2, the 1 means

a)

there is 1 electron

b)

the electrons are in the 1st energy level

c)

the shape is circular

d)

there is a -1 charge

21.

In 1s2, the s means

a)

the shape of the orbital is circular

b)

the shape of the orbital is figure 8

c)

there are six electrons

d)

it is neutral

22.

In 1s2, the 2 means

a)

there are 2 electrons in this level

b)

it is the 2nd energy level

c)

there is a +2 charge

d)

there is a -2 charge

23.

What is the suitable correction for 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 another one arrow should be in the 2nd 2p box.

d)

All the arrows should be pointing up.

24.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
25.

Which orbital shows a violation of the Aufbau Principle?

a)

A

b)

B

c)

C

d)

D

26.
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
27.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

28.

Where electrons can be found?

a)

Outside the nucleus

b)

Under my bed

c)

Inside the nucleus

d)

Inside a proton

29.

What are the maximum number of electrons in the first 3 energy levels?

a)

2,4,16

b)

2,8,18

c)

4,8,12

d)

3,4,6

30.
What are valence electrons?
a)
electrons on the first orbital always
b)
nucleus
c)
the outermost shell
d)
the number of electrons on the outermost orbital
31.
Which particles make up the nucleus of an atom?
a)
protons and neutrons
b)
electrons and protons
c)
electrons, protons, and neutrons
d)
electrons and neutrons
32.
What is the maximum number of electrons that can be contained in the 2nd energy level?
a)
2
b)
6
c)
8
d)
18
33.
How many sublevels are there? 
a)
1
b)
2
c)
3
d)
4
34.
Which among the following sublevels must be filled up first?
a)
s-sublevel
b)
p-sublevel
c)
d-sublevel
d)
f-sublevel
35.
How many orbitals are present in the p-sublevel?
a)
1
b)
3
c)
6
d)
9
36.
How many orbitals are in the d-sublevel?
a)
2
b)
3
c)
5
d)
10
37.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
38.

What is the shape of a p orbital?

a)

sphere

b)

it's just too complex to think about it

c)

dumbbell

d)

I don't know this stuff.

39.

Which two of these answers would have the same shape?

a)

2p

b)

2s

c)

3d

d)

1s

40.

What are the 4 quantum numbers for the 8th electron in 1s2 2s2 2p6 ?

a)

(2, 1, 0, 1/2)

b)

(1, 0, 0, -1.2)

c)

(2, 1, -1, -1/2)

d)

(2, 1, -1, 1/2)

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