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Long Quiz in Science 9

Total questions: 50

Worksheet time: 38mins

Name
Class
Date
1.

Which orbital designation has the highest energy?

a)

2p

b)

2s

c)

3d

d)

4s

2.

The symbol “n” in the Bohr theory of atomic structure refers to _______.

a)

the energy of electron

b)

the orbit in which an electron is found

c)

the total energy of the atom

d)

the number of electrons in an energy level

3.

How many electrons occupy the 3d orbitals in atoms when it is completely filled?

a)

2

b)

3

c)

6

d)

10

4.

What kind of bond will result when two identical non-metallic atoms combine?

a)

ionic bond

b)

metallic bond

c)

non metal bond

d)

covalent bond

5.

Why do atoms react with one another to form chemical bonds?

a)

to attain stability

b)

to produce ions

c)

to form molecules

d)

to form compounds

6.

Who proposed the nuclear model of the atom?

a)

Bohr

b)

Dalton

c)

Rutherford

d)

Schrödinger

7.

Which model explains electron behavior using waves?

a)

Quantum mechanical model

b)

Planetary model

c)

Plum pudding model

d)

Solid sphere model

8.

The modern atomic model is based on:

a)

Classical mechanics

b)

Quantum mechanics

c)

Planetary motion

d)

Chemical bonding

9.

Who introduced the concept of electron clouds?

a)

Bohr

b)

Schrödinger

c)

Dalton

d)

Rutherford

10.

Quantum numbers describe:

a)

Atomic mass

b)

Electron properties and behavior

c)

Number of neutrons

d)

Chemical symbols

11.

How many quantum numbers describe an electron completely?

a)

2

b)

3

c)

4

d)

5

12.

The principal quantum number (n) describes:

a)

Energy level

b)

Shape

c)

Orientation

d)

Spin

13.

The angular momentum quantum number (l) indicates:

a)

Energy level

b)

Shape of orbital

c)

Spin direction

d)

Magnetic field

14.

The magnetic quantum number (ml) describes:

a)

Orientation of the orbital

b)

Size of the atom

c)

Energy of the nucleus

d)

Spin of the electron

15.

The spin quantum number (ms) shows:

a)

Electron charge

b)

Spin direction

c)

Energy level

d)

Shape

16.

What is the maximum number of electrons in the s orbital?

a)

1

b)

2

c)

3

d)

6

17.

The f sublevel can hold a maximum of:

a)

6

b)

10

c)

14

d)

18

18.

The orbital that looks like a dumbbell shape is:

a)

s

b)

p

c)

d

d)

f

19.

The orbital shape represented by a sphere is:

a)

s

b)

p

c)

d

d)

f

20.

Electron configuration refers to:

a)

Distribution of neutrons

b)

Arrangement of electrons in orbitals

c)

Location of protons

d)

Shape of atoms

21.

What does the atomic number represent?

a)

Number of neutrons

b)

Number of electrons and protons

c)

Atomic mass

d)

Energy level

22.

The electron configuration of hydrogen is:

a)

1s¹

b)

1s²

c)

2s¹

d)

2p¹

23.

The electron configuration of helium is:

a)

1s¹

b)

1s²

c)

2s²

d)

2p⁶

24.

Sodium (Na) has how many electrons?

a)

10

b)

11

c)

12

d)

13

25.

The electron configuration of sodium is:

a)

1s² 2s² 2p⁶ 3s¹

b)

1s² 2s² 2p⁶

c)

1s² 2s² 3s²

d)

1s² 2p⁶ 3s¹

26.

Which element has the configuration 1s² 2s² 2p⁶ 3s² 3p⁶?

a)

Neon

b)

Argon

c)

Sodium

d)

Potassium

27.

Krypton's electron configuration ends with:

a)

4p⁶

b)

4s²

c)

3p⁶

d)

3d¹⁰

28.

Which element has 10 electrons?

a)

Neon

b)

Sodium

c)

Aluminum

d)

Oxygen

29.

A chemical bond is the force that:

a)

Separates atoms

b)

Holds atoms together

c)

Destroys molecules

d)

Increases atomic mass

30.

What causes atoms to form bonds?

a)

To gain protons

b)

To achieve stability

c)

To lose neutrons

d)

To form isotopes

31.

Ionic bonds occur between:

a)

Metal + Metal

b)

Nonmetal + Nonmetal

c)

Metal + Nonmetal

d)

Noble gases

32.

Covalent bonds occur between:

a)

Metal + Metal

b)

Metal + Nonmetal

c)

Nonmetal + Nonmetal

d)

Noble gases

33.

In an ionic bond, electrons are:

a)

Shared equally

b)

Transferred

c)

Lost by both atoms

d)

Split in half

34.

In a covalent bond, electrons are:

a)

Lost

b)

Shared

c)

Gained

d)

Neutralized

35.

Is CaF an ionic or covalent compound?

a)

Ionic

b)

Covalent

36.

Is CH an ionic or covalent compound?

a)

Ionic

b)

Covalent

37.

Is AlCl an ionic or covalent compound?

a)

Ionic

b)

Covalent

38.

Is HNO an ionic or covalent compound?

a)

Ionic

b)

Covalent

39.

Is KSO an ionic or covalent compound?

a)

Ionic

b)

Covalent

40.

Identify whether the element Antimony is a metal, non-metal, or metalloid (semi metal).

a)

Metal

b)

Non-Metal

c)

Semi Metal

41.

Identify whether the element Iodine is a metal, non-metal, or metalloid (semi metal).

a)

A – Metal

b)

B – Non-Metal

c)

C – Semi Metal

42.

Identify whether the element Potassium is a metal, non-metal, or metalloid (semi metal).

a)

Metal

b)

Non-Metal

c)

Semi Metal

43.

Identify whether the element Zinc is a metal, non-metal, or metalloid (semi metal).

a)

Metal

b)

Non-Metal

c)

Semi Metal

44.

Identify whether the element Iron is a metal, non-metal, or metalloid (semi metal).

a)

Metal

b)

Non-Metal

c)

Semi Metal

45.

Identify whether the element Tellurium is a metal, non-metal, or metalloid (semi metal).

a)

A – Metal

b)

B – Non-Metal

c)

C – Semi Metal

46.

What is the Electron Configuration of Hydrogen

a)

1s¹

b)

1s²

c)

2s¹

d)

2p¹

47.

What is the electron configuration for Lithium.

a)

1s² 2s¹

b)

1s² 2p¹

c)

1s¹ 2s²

d)

1s² 2s²

48.

Write the electron configuration for Boron.

a)

1s² 2s² 2p¹

b)

1s² 2s² 2p³

c)

1s² 2s¹ 2p²

d)

1s² 2p³

49.

Write the electron configuration for Oxygen.

a)

1s² 2s² 2p⁴

b)

1s² 2s² 2p⁶

c)

1s² 2s² 2p²

d)

1s² 2s² 2p³

50.

What is the element COnfiguration for Aluminum

a)

1s² 2s² 2p⁶ 3s² 3p¹

b)

1s² 2s² 2p⁶ 3s² 3p⁵

c)

1s² 2s² 2p⁶ 3s² 3p³

d)

1s² 2s² 2p⁶ 3s² 3p⁶

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