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9th chem term 1

Total questions: 114

Worksheet time: 1hrs 28mins

Name
Class
Date
1.

what charge does the nucleus have

a)

negative

b)

neutral

c)

positive

d)

none of the above

2.

name the 3 subatomic particles

a)

proton

b)

nucleus

c)

neutron

d)

electron

3.

the function of a neutron is to keep the protons in the nucleus from repelling away from each other

a)

True

b)

False

4.

why do the electrons not crash into the nucleus

a)

they repel from the nucleus

b)

they are going to fast

c)

they dont move so they cant crash into the nuceleus

5.

what does it mean for an atom to be stable

a)

to have the same number of protons as neutrons

b)

to have a lot of electrons

c)

to have little protons

d)

to not have a nucleus

6.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
7.

What is this element?

a)

Beryllium (atomic #4)

b)

Boron (atomic #5)

c)

Carbon (atomic #6)

d)

Nitrogen (atomic #7)

8.

In the Bohr model, how do electrons travel?

a)

Electrons move in and out of the nucleus

b)

Electrons do not move

c)

Electrons move in circular orbits around the nucleus

d)

Electrons move in a straight line

9.

Which of the following is the first postulate of Bohr's atomic model?

a)

Electron moves in circular orbits around the nucleus

b)

The energy of an electron in a hydrogen atom is quantised

c)

If energy is supplied, electron absorbs the energy and is promoted from a lower energy level to a higher energy level

d)

At excited state, the electron is unstable. It will fall back to lower energy level and releases a specific amount of energy (photon) in the form of light

10.
He discovered the neutron in the nucleus and completed the current atomic model.
a)
J.J. Thomson
b)
Ernest Rutherford
c)
Niels Bohr
d)
James CHadwick
11.
He found that atoms have smaller parts and found negative electrons that he theorized were surrounded in a sphere of positive charges
a)
J.J. Thomson
b)
Ernest Rutherford
c)
Niels Bohr
d)
James Chadwick
12.
He found the positively charged protons in the nucleus and said that electrons moved around the nucleus
a)
J.J. Thomson
b)
Ernest Rutherford
c)
Niels Bohr
d)
James Chadwick
13.
He found that electrons have specific amounts of energy and move in specific orbits around the nucleus, like planets orbiting the sun. 
a)
J.J. Thomson
b)
Ernest Rutherford
c)
Niels Bohr
d)
James Chadwick
14.
According to Ernest Rutherford, an atom is made of mostly....
a)
empty space
b)
electrons
c)
the nucleus
d)
protons
15.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
16.
How are electrons arranged in an atom?
a)
In groups of five
b)
In energy levels
c)
By color
d)
By shape
17.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
Electrons and megatrons
18.

Which element does this Bohr model represent?

a)

Aluminum

b)

Silicon

c)

Magnesium

d)

Cobalt

19.

What is the mass of this atom?

a)

9

b)

10

c)

19

d)

28

20.

How many neutrons does this element have?

a)

45

b)

80

c)

35

d)

7

21.

Electron live in something called __________.

a)

nucleus

b)

orbits

c)

Shells or Energy levels

d)

Valences

22.
What is the tiny, massive central part of the atom?
a)
Neutron
b)
Electron
c)
Proton
d)
Nucleus
23.
Whose model is most similar to the solar system?
a)
Bohr
b)
Thomson
c)
Rutherford
d)
Dalton
24.
When an element loses an electron, it becomes a
a)
ion
b)
isotope
c)
decay
d)
new element
25.
When an element loses an electron, it becomes?
a)
positive
b)
negative
c)
neutral
d)
a new element
26.

Who first had evidence of the atom?

a)

Bohr

b)

Dalton

c)

Rutherford

d)

Thompson

27.

Who discovered the electron?

a)

Bohr

b)

Dalton

c)

Rutherford

d)

Thompson

28.

Who's model does this picture represent?

a)

Dalton 1803-1808

b)

Thomson 1897

c)

Rutherford 1911

d)

Bohr 1913

29.

Who's model does this picture represent?

a)

Dalton 1803-1808

b)

Rutherford 1911

c)

Thomson 1897

d)

modern atomic model 1920 to the present

30.

Who's model does this represent?

a)

Dalton 1903-1808

b)

Rutherford 1911

c)

Thomson 1897

d)

Bohr 1913

31.

What is the shape of p orbitals?

a)

Peanut shaped

b)

Spherical shaped

c)

Flower shaped

d)

Dumbbell shaped

32.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
33.
What is the maximum number of electrons that can be on the p sublevel?
a)
6
b)
3
c)
2
d)
4
34.

What shape are d orbitals?

a)

Peanut shaped

b)

Spherical shaped

c)

Dumbbell shaped

d)

Clove leaf shaped

35.
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
36.
Hund’s rule states…
a)
Atomic orbitals have opposite spins and 2 electrons each
b)
Electrons occupy orbitals of highest energy first and energy level changes as you go up
c)
Electrons occupy orbitals of lowest energy first, starting with 1s
d)
Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.
37.
How many orbitals are there in the "d" sublevel?
a)
1
b)
3
c)
5
d)
7
38.
How many orbitals are there in the "s" sublevel?
a)
1
b)
3
c)
5
d)
7
39.
Which sublevel has the highest energy?
a)
3s
b)
3d
c)
3p
40.
The Quantum Mechanical Model is the most recent/modern atomic model.
a)
True
b)
False
41.
The quantum number "n" represents:
a)
electron spin
b)
orbital
c)
sublevel
d)
main energy level
42.

Which scientist developed the Quantum Mechanical

a)

E. Schroedinger

b)

Rutherford

c)

J. Dalton

d)

N. Bohr

43.
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
44.

If the first and second energy levels of an atom are full, then what would be the total number of electrons in the atom?

a)

6

b)

8

c)

10

d)

18

45.

Which of the following sub-levels is correctly designated?

a)

1p5

b)

3f9

c)

2p6

d)

3d11

46.

Which of the following statement is wrong?

a)

Two electrons must occupy each equal energy orbital before additional electrons can occupy the same orbitals.

b)

A maximum of two electrons may occupy the same orbitals.

c)

In filling up orbitals, electron occupies the lowest energy orbital first before the higher energy orbitals.

d)

None of the choices.

47.

What is the electron configuration of Argon?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s1

c)

1s2 2s2 2p6 3s2

d)

1s2 2s2 2p6 3s2 3p6

48.

What is the electron configuration of Gallium, 31Ga?

a)

1s2 2s2 2p6 3s2 3p5 4s2 3d10 4p1

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d9 4p2

d)

1s2 2s2 2p6 3s2 3p5 4s2 3d10 4p2

49.

Which one of the following electron configurations is INCORRECT?

a)

1s2 2s2 2p6 3s2 3p6

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d9 4p2

50.

Which of the following electron configurations is CORRECT?

a)

1s2 2s3

b)

1s2 2s2 2p6

c)

1s2 2s2 3s2

d)

1s2 2s2 2p6 3s2 4s2

51.

Chalcogens belongs to

a)

group 15

b)

group 16

c)

group 17

d)

group 18

52.

Choose the s-block element in the following :

a)

1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s1

b)

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

c)

1s2, 2s2, 2p6, 3s2, 3p6, 4s1

d)

all of the above

53.

Representative elements are those which belong to

a)

p and d – Block

b)

s and d – Block

c)

s and p – Block

d)

s and f – Block

54.

The group number, number of valence electrons, and valency of an element with the atomic number 15, respectively, are:

a)

6, 5 and 2

b)

15, 5 and 3

c)

16, 6 and 3

d)

15, 6 and 2

55.

In the modern periodic table, the period indicates the value of:

a)

Atomic Number

b)

Atomic Mass

c)

Principal Quantum Number

d)

Azimuthal Quantum Number

56.

In the long form of the periodic table, the valence shell electronic configuration of 5s²5p4 corresponds to the element present in:

a)

Group 16 and period 6

b)

Group 17 and period 6

c)

Group 16 and period 5

d)

Group 17 and period 5

57.

The number of elements in the 5th period of the periodic table is

a)

2

b)

8

c)

18

d)

32

58.

The electronic configuration of halogen is

a)

ns² np6

b)

ns² np3

c)

ns² np5

d)

ns²

59.

first group elements are named as

a)

alkali metals

b)

alkaline earth metals

c)

chalcogens

d)

halogens

60.

d-block element form

a)

ionic compounds

b)

covalent compounds

c)

both ionic and covalent compounds

d)

ionic , coordination and covalent compounds

61.

Which group elements have high melting points and are good conductors of heat and electricity.

a)

s-block

b)

p-block

c)

d-block

d)

f-block

62.

Which group shows variable oxidation states

a)

s block

b)

d block

c)

f block

d)

both f and d block

63.

The group of elements in which the differentiating electron enters the anti penultimate shell of atoms are called

a)

s block elements

b)

p block elements

c)

d block elements

d)

f block elements

64.

1.What would be the IUPAC name for an element with atomic number 112?

a)

bibibiium

b)

dibibiium

c)

unibibiium

d)

uniunibiium

65.

the first inner transition series starts in---period

a)

3

b)

4

c)

5

d)

6

66.

Elements in the Modern Periodic table are arranged in order of___

a)

Decreasing atomic number

b)

Decreasing atomic mass

c)

Increasing atomic number

d)

Increasing atomic mass

67.

Modern periodic law had been given by ____

a)

Moseley

b)

Mendeleev

c)

Lavoisier

d)

Lother-Mayer

68.

How many periods and groups are present in the periodic table?

a)

7 periods and 18 groups

b)

8 periods and 7 groups

c)

7 periods and 7 groups

d)

8 periods and 8 groups

69.

The elements in group zero are called___

a)

Alkali metals

b)

Transition metals

c)

Inert gases

d)

Alkali Earth metals

70.

In periodic table elements with same number of shells/orbits are placed in___

a)

Different groups

b)

same groups

c)

same periods

d)

different periods

71.

Which of the following elements has 2 shells and both are completely filled?

a)

Helium

b)

Neon

c)

Calcium

d)

Boron

72.

Transition metals are found between group number___

a)

1 to 2

b)

13 to 18

c)

3 to 12

d)

1 to 8

73.

An element X belongs to the 3rd period and 1st group of the periodic table. What is the number of valence electrons in its atom?

a)

1

b)

3

c)

6

d)

8

74.

An element M is in group 13th of the periodic table, the formula for its oxide is

a)

MO

b)

M2O3

c)

M3O2

d)

MO2

75.
The atomic number of an element tells the number of _____ in the nucleus of an atom of that element.
a)
protons
b)
neutrons
c)
electrons
d)
isotopes
76.

What period is Lead (Pb) in?

a)

6

b)

4

c)

Metals

d)

4A

77.

What category is silicon (Si) a part of?

a)

Metal

b)

Nonmetal

c)

Metalloid

d)

Halogens

78.

What Element is in period 4, group 5A/15?

a)

Antimony

b)

Arsenic

c)

Tin

d)

Germanium

79.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
80.
How did Mendeleev arrange the elements?
a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
81.

What is the oxidation state of Cl in ClO- ?

a)

0

b)

+1

c)

-1

d)

+2

82.

What is the oxidation state of Cu in Cu2+?

a)

-1

b)

-2

c)

+2

d)

0

83.

What is the oxidation state of H in H2?

a)

+2

b)

+1

c)

0

d)

None of the above

84.

What is the oxidation state of Pb in PbO ?

a)

+2

b)

+4

c)

0

d)

-2

85.

C in CO32-?

a)

-4

b)

+2

c)

0

d)

+4

86.

S in HSO4- ?

a)

+5

b)

-6

c)

+6

d)

+2

87.

H in NaH ?

a)

+1

b)

0

c)

-1

d)

None of the above

88.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2
89.
What is the oxidation number of O in CO2?
a)
+2
b)
-1
c)
+4
d)
-2
90.
What is the oxidation number of N in NO21- ?
a)
-3
b)
+4
c)
-2
d)
+3
91.
What is the oxidation of C in CH4?
a)
-4
b)
-1
c)
+4
d)
+1
92.
What is oxidation number of Mn in MnO2 ?
a)
0
b)
+2
c)
-2
d)
+4
93.
What is the oxidation number of Ca in Ca3N2?
a)
+3
b)
+2
c)
-3
d)
-2
94.
What is oxidation number of Cr in
Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
95.

The valence electron can

a)

Cannot interact in a chemical reaction.

b)

Can interact in a chemical reaction.

96.

Atoms are electrically neutral when

a)

They have a minimal charge.

b)

They have a balanced number of protons and neutrons.

c)

They have a balanced number of protons and electrons.

d)

They have no valance electrons.

97.

If an electron is removed, an ion becomes

a)

An atom

b)

Positive

c)

Negative

d)

Neutral

98.

Cations have what type of charge?

a)

Positive

b)

Negative

99.

What is the charge of Iron(III)

a)

+3

b)

+1

c)

+2

d)

+4

100.

ALL anions are

a)

Metal

b)

Transitional Metals

c)

Nobel Gases

d)

Non-Metal

101.

What is the formula of an ionic compound formed from Lithium and Oxygen?

a)

Li2O

b)

LiO2

c)

2LiO

d)

Li2O

102.

What is the name of an ionic compound formed from Calcium and Oxygen?

a)

Calcium Oxide

b)

Calcium Monoxide

c)

Monocalcium Monoxide.

d)

Calcium Dioxide

103.

What is the chemical formula of sodium sulfate?

a)

SSO4

b)

SoSO4

c)

NaSO4

d)

Na2SO4

104.

What is the formula of Copper (II) oxide?

a)

CUO

b)

CuO

c)

CuO2

d)

Cu2O

105.

How many atoms are there in the compound MgCO3?

a)

3

b)

4

c)

5

d)

6

106.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
107.

How many electrons are there in the valence shell of the O2– ion?

a)

2

b)

8

c)

10

d)

6

108.
Diagram below shows
a)
formation of hybrid orbital
b)
atomic orbital overlap to produce hybrid orbital
c)
atomic orbital overlap to form sp hybrid orbital
d)
s orbital overlap with p orbital to form sp hybrid orbital
109.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
110.

20. If I was trying to determine if two atoms will bond, what would be helpful to know:

a)

Valence electrons, found by group number

b)

Whether the elements are metals or nonmetals

c)

The electronegativity of the atoms

d)

All of the above, all of which can be found on the Periodic Table

111.

Predict the bond between Mg and Cl

a)

covalent

b)

ionic

c)

metallic

d)

none of the above

112.

Which is the correct Lewis Structure for oxygen?

a)
b)
c)
d)
113.

What is the correct Lewis structure for BF3?

a)
b)
c)
d)

BF3 (The formula is the Lewis Structure)

114.
Using electronegativities, what type of bond is formed by S and Br.
a)
ionic
b)
polar covalent
c)
non-polar covalent

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