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Chapter 2 chemistry

Total questions: 30

Worksheet time: 14mins

Name
Class
Date
1.
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
2.
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
3.
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
4.

How many electrons can an energy level of n = 2 hold?

a)

32

b)

24

c)

8

d)

6

5.

What are the shapes of p orbitals ?

a)

cloverleaf

b)

spherical

c)

dumbbell

6.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
7.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
8.

Chemists can identify the composition of some unknown salts by conducting a flame test. When potassium salts are heated in a flame, a purple color is observed.


This is due to the movement of electrons between energy levels. What is the electron configuration of a potassium atom at ground state?

a)

1s2; 2s2; 2p6; 3s2; 3p6; 4d1

b)

1s2; 2s2; 2p6; 3s2;3p6; 3d1

c)

1s2; 2s2; 2d6; 3s2; 3d6; 4s1

d)

1s2; 2s2; 2p6; 3s2; 3p6; 4s1

9.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
10.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
11.

2. A quantum number determining orbital orientation around the atom’s core is called... .

a)

n

b)

l

c)

m

d)

s

12.

3. A subshell containsing 7 orbitals is called ... subshell.

a)

s

b)

p

c)

d

d)

f

13.

4. Below are the examples on how to fill the atomic quantum number, except... .

a)

n = 2, l =1, m = 0, s = -1/2

b)

n = 1, l =3, m = 0, s = +1/2

c)

n = 3, l =1, m = 0, s = -1/2

d)

n = 3, l = 2, m = +2, l = +1/2

14.

7. The magnetic quantum number (m), has value within... .

a)

0 up to (n-1)

b)

0, 1, 2, 3, ...

c)

-l up to. +l

d)

-1/2 and +1/2

15.

15. Orbital shape of an atom is characterized by ... quantum number.

a)

Spin projection

b)

Primal

c)

Magnetic

d)

Azimuthal

16.
Which section of the spectrum is the ONLY one we can see?
a)
X-rays
b)
Visible Light
c)
Gamma Rays
d)
Ultraviolet Rays
17.
As the frequency of an electromagnetic wave increases, the amount of energy in that wave...
a)
increases.
b)
decreases.
c)
stays the same.
18.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
19.

Which the equation show the relationship among wavelength, frequency, and speed of radiation.

a)

ΔE =hcλ\Delta E\ =\frac{hc}{\lambda}

b)

ΔE=hv\Delta E=hv

c)

λ = cv\lambda\ =\ \frac{c}{v}

d)

En=− RH (1n2)En=-\ R_{H\ }\left(\frac{1}{n^2}\right)

20.

Bohr's idea about the atom is pretty good, however it has limitation. What is this limitation?

a)

It lacks substantial evidence explaining the spectral lines of the Hydrogen atom.

b)

His model is too simple.

c)

His model can no longer explain the behavior of electron based on its spectral lines of atoms with more than one electron.

d)

None of the above

21.

According to Bohr, the energy absorbed by an electron upon excitation comes in a fixed amount called

a)

exact energy

b)

fixed energy

c)

quantized energy

d)

None of the above

22.

the diagram show

a)

the formation of continous spectrum

b)

the formation of line spectrum

23.

Which the energy of an electron in a given energy state of the H atom.

a)

ΔE =hcλ\Delta E\ =\frac{hc}{\lambda}

b)

ΔE=hv\Delta E=hv

c)

λ = cv\lambda\ =\ \frac{c}{v}

d)

En=− RH (1n2)En=-\ R_{H\ }\left(\frac{1}{n^2}\right)

24.
A line spectrum is produced when an electron moves from one energy level
a)
into the nucleus.
b)
to another position in the same sublevel.
c)
to a higher energy level.
d)
to a lower energy level.
25.
Electrons act as both
a)
Energy and Light
b)
Neutrons and photons
c)
Positives and negatives
d)
Particles and waves
26.

Which of the following line is correct when electron undergoes transition from excited state n= 7 to ground state n= 1 in Lyman Series

a)

5th line

b)

4th line

c)

6th line

d)

7th line

27.

transition of electron from an excited state to a ground state of n = 5 formed a photon. Which of the following series belongs to this respective transition?

a)

Balmer

b)

Pfund

c)

Brackett

d)

Lyman

e)

Paschen

28.

choose the correct line spectrum formed when electron falls down from n=5 to n =3

a)

3rd line

b)

1st line

c)

2nd line

d)

4th line

29.

If energy is supplied, electron ___________ the energy and is _____________ from a lower energy level to a higher ones.

a)

absorbed, promoted

b)

emitted, promoted

c)

absorbed, demoted

d)

emitted, demoted

30.

At excited state electron is _______________and it will fall back to lower energy level and released a specific amount of ________________ in form of light (photon).

a)

unstable, energy

b)

stable, wavelength

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