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CHEM 20A Final Review

Total questions: 55

Worksheet time: 44mins

Name
Class
Date
1.

An unused flashbulb contains magnesium and oxygen. After use, the contents are changed to magnesium oxide but the total mass does not change. This observation can best be explained by the

a)

Law of Constant Composition

b)

Law of Multiple Proportions

c)

Avogadro's Law

d)

Law of Conservation of Mass

2.

Can form +2 charge when ionized

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble gas

3.

How many moles in in 0.890g of fluorine gas?

a)

0.0234 mol

b)

0.0468 mol

c)

33.8 mol

d)

16.9 mol

4.

Which of the following contains smallest number of molecules?

a)

5.0g CO2

b)

5.0g O2

c)

5.0g H2

d)

5.0g N2

5.

How many aluminum atoms are there in 3.50 grams of Al2O3?

a)

4.13 x 1022

b)

4.90 x 1022

c)

2.07 x 1022

d)

1.68 x 1022

6.

Balance the following chemical equations: _Al + _H2SO4 -> _Al2(SO4)3 + _H2

a)

2, 2, 1, 3

b)

4, 3, 1, 3

c)

2, 3, 1, 3

d)

2, 3, 2, 3

7.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
8.

For 2Al + 6HCl -> Al2Cl6 + 3H2, calculate the mass of H2 formed when 25g of Al reacted.

a)

0.41g

b)

1.2g

c)

1.8g

d)

2.8g

9.

Rutherford carried out experiments in which a beam of alpha particles was directed at a thin piece of metal foil. From these experiments he concluded that:

a)

electrons are massive particles.

b)

the positively charged parts of atoms are moving about with a velocity approaching the speed of light.

c)

the positively charged parts of atoms are extremely small and extremely heavy particles.

d)

the diameter of an electron is approximately equal to that of the nucleus.

e)

electrons travel in circular orbits around the nucleus.

10.

What is the wavelength range of the visible spectrum?

a)

1mm - 1m

b)

780 nm - 1mm

c)

400 nm - 700 nm

d)

100 nm - 400 nm

11.

When the frequency of electromagnetic radiation increases, the speed of radiation increases.

a)

True

b)

False

12.

Which of the following properties does not affect the photoelectric effect?

a)

Kinetic energy

b)

Work function

c)

Light intensity

d)

Wavelength

13.

The energy of the radiation is proportional to the wavelength.

a)

True

b)

False

14.

Increasing the wavelength of incoming light increases the kinetic energy of the ejected electrons

a)

True

b)

False

15.

According to Bohr Theory, which of the following transitions in the hydrogen atom will give rise to the least energetic photon?

Use the equation: En = (-2.18 x 10-18 J)(1/n2)

a)

n = 5 to n = 3

b)

n = 6 to n = 1

c)

n = 4 to n = 3

d)

n = 6 to n = 5

16.

What is the frequency of light having a wavelength of 4.50 x 10-6 cm?

a)

2.84 x 10-12 s-1

b)

2.10 x 104 s-1

c)

4.29 x 1014 s-1

d)

6.67 x 1015 s-1

17.

The work function is the minimum energy required to eject an electron from a metal surface

a)

True

b)

False

18.

Effective nuclear charge generally increases from left to right in a period and top to bottom in a group

a)

True

b)

False

19.

Shorter bonds are stronger bonds with larger bond energy

a)

True

b)

False

20.

Which of the following require least energy to break the bond?

a)

single bond

b)

double bond

c)

triple bond

21.

Which molecule has a linear arrangement of all component atoms?

a)

CH4

b)

H2O

c)

CO2

d)

NH3

22.

Ionization energy increases from left to right in a period

a)

True

b)

False

23.

Atomic radius increases from left to right in a period

a)

True

b)

False

24.

Elements in the same period have the same number of

a)

valence electrons

b)

protons

c)

electrons

d)

energy levels

25.

An atom with atomic radius smaller than sulfur is

a)

O

b)

Cl

c)

Ca

d)

Li

26.

The ionization energy of Na is greater than Li

a)

True

b)

False

27.

The atomic radius of Be is smaller than Mg

a)

True

b)

False

28.

He has a higher ionization energy than Nitrogen

a)

True

b)

False

29.

Sulfur is more electronegative than Selenium

a)

True

b)

False

30.

What is the electron configuration of Fe3+?

a)

[Ar]3d64s2

b)

[Ar]3d5

c)

[Ar]3d64s24p3

d)

[Ar]3d6

31.

The valence electrons of representative elements are

a)

in s orbitals only.

b)

located in the outermost occupied major energy level.

c)

located closest to the nucleus

d)

located in d orbitals.

32.

Which of the following pairs of elements and valence electrons is incorrect?

a)

Al - 3

b)

Br - 7

c)

S - 4

d)

Sr - 2

33.

In the Schrodinger wave equation, ψ represents

a)

Orbitals

b)

wavefunctions

c)

amplitude functions

d)

wavefunctions and amplitude

e)

all of the above

34.

The Schrodinger wave equation is a mathematical expression describing

a)

energy of the electron

b)

momentum of the electron

c)

position of the electron

d)

All of the above

35.
Why do atoms share electrons?
a)
To attain the electron configuration of a noble gas.
b)
To become ions and take a charge
c)
to increase the mass
d)
it's a nice thing to do.
36.

A π (pi) bond is the result of the

a)

overlap of two s orbitals.

b)

overlap of an s and a p orbital.

c)

overlap of two p orbitals along their axes.

d)

sidewise overlap of two parallel p orbitals.

e)

sidewise overlap of two s orbitals.

37.

If the electron configuration of an element is 1s2 2s2 2p6 3s2 3p5, it is

a)

S

b)

Br

c)

Cl

d)

P

38.

Once the electron in a hydrogen atom absorbs energy, it

a)

is now in its ground state

b)

is now in its excited state

c)

has released a photon

d)

none of the above

39.

The first 3 electron entering p orbitals must have

a)

opposite spins

b)

opposite charges

c)

parallel spins

d)

low energy levels

40.

The energy of the particle in a box is proportional to __________

a)

n

b)

n-1

c)

n2

d)

n-2

41.

Which of the following atomic orbital is impossible?

a)

2p

b)

4f

c)

3s

d)

2d

42.

The electron configuration of chromium ion is [Ar]3d4, what is the charge?

a)

3-

b)

3+

c)

2+

d)

2-

43.

Which quantum number represents the shape of an orbital?

a)

n

b)

l

c)

ml

d)

ms

44.

The maximum number of electrons that can occupy n = 3 level is

a)

18

b)

32

c)

10

d)

8

45.

In order to occupy the same orbital, 2 electrons must have

a)

same direction of spin

b)

low energy

c)

opposite charge

d)

opposite spin

46.

Which of the following orbitals can be represented by the set of quantum numbers (n = 4), (l = 1), (ml = -1), (ms = 1/2)?

a)

4d

b)

4p

c)

4s

d)

not possible

47.

According to the Aufbau principle, the electron occupies that sub-shell with the

a)

lowest energy

b)

highest energy

c)

zero energy

d)

none of the above

48.

In the ground state of a cobalt atom there are _____ unpaired electrons and the atom is _____.

a)

3, paramagnetic

b)

5, paramagnetic

c)

2, diamagnetic

d)

0, diamagnetic

49.

Antibonding molecular orbitals are produced by

a)

constructive interaction of atomic orbitals.

b)

destructive interaction of atomic orbitals.

c)

the overlap of the atomic orbitals of two negative ion

d)

none of the above

50.

What kind of molecular orbital forms when the two atomic orbitals shown below interact in the manner indicated?


a)

σ

b)

σ*

c)

π

d)

π*

51.

What kind of molecular orbital forms when the two atomic orbitals shown below interact in the manner indicated?

a)

σ

b)

σ*

c)

π

d)

π*

52.

What is the bond order of O2+?

a)

1

b)

1.5

c)

2

d)

2.5

53.

Draw the molecular orbital diagram for the molecular ion, N2+. The number of electrons in the σ2p molecular orbital is:

a)

1

b)

2

c)

3

d)

4

54.

Draw the molecular orbital diagram for B2. The number of unpaired electrons in the B2 molecule is

a)

0

b)

1

c)

2

d)

3

55.

(Crystal Field Theory) When the valence d orbitals of the central metal ion are split in energy in an octahedral ligand field, which orbitals are raised least in energy?

a)

dxy and dx2-y2

b)

dxy, dxz and dyz

c)

dxz and dyz

d)

dxz, dyz and dz2

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