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T1-Final Science Revision Quiz

Total questions: 83

Worksheet time: 4hrs 25mins

Name
Class
Date
1.

In an element box, the number at top is the

a)

atomic number

b)

atomic name

c)

atomic mass

d)

atomic symbol

2.

The number of neutrons in an atom can be found by

a)

adding the number of neutrons and protons together.

b)

adding the atomic mass and the atomic number.

c)

subtratcting the atomic number from the atomic mass.

d)

subtracting the atomic mass from the atomic number.

3.

___________________ are positively charged particles located in the nucleus of an atom.

a)

Electrons

b)

Neutrons

c)

Protons

d)

Isotopes

4.

Isotopes are atoms of the same element with different numbers of

a)

electrons

b)

neutrons

c)

protons

d)

nuclei

5.

Elements on the Periodic Table are ordered according to their

a)

element name

b)

element symbol

c)

number of atoms

d)

atomic number

6.

Rows in the Periodic Table are called

a)

Periods

b)

Groups/Families

c)

Cousins

d)

Metals

7.

Rows in the Periodic Table are called

a)

Periods

b)

Groups/Families

c)

Cousins

d)

Metals

8.

Column in the Periodic Table are called

a)

Periods

b)

Groups/Families

c)

Cousins

d)

Metals

9.

The elements that touch the zigzag line on the Periodic Table are called

a)

metals

b)

nonmetals

c)

metalloids

d)

gasses

10.

The nucleus of an atom is located in its

a)

electron cloud

b)

center

c)

proton

d)

backpack

11.

What do atoms of the same periodic group have in common?

a)

They have the same atomic number.

b)

They have the same chemical symbols.

c)

The have similar chemical properties.

d)

They have the same atomic mass.

12.

The smallest particle of an element that has the same chemical properties of the element is

a)

a molecule of that element.

b)

an atom of that element.

c)

a proton of that element.

d)

the nucleus of the element.

13.

Protons have a ____________ charge, neutrons have a ____________ charge, and electrons have a ____________ charge.

a)

positive; negative, neutral

b)

positive, neutral, negative

c)

neutral, negative, positive

d)

negative, neutral, positive

14.

The chemical symbol in this element box is

a)

26

b)

Fe

c)

Iron

d)

55.845

15.

The three kinds of elements are

a)

metals, nonmetals, and liquid metals

b)

metals, nonmetals, and metalloids

c)

metals, solids, and liquids

d)

metalloids, asteroids, and nonmetals

16.

The Periodic Table of elements is arranged according to an element's

a)

color

b)

state of matter

c)

place in the alphabet

d)

properties

17.

All matter is made of

a)

electrons

b)

protons

c)

neutrons

d)

atoms

18.

Most elements on the periodic table are classified as ____________.

a)

Gases

b)

Metalloids

c)

Metals

d)

Nonmetals

19.

Groups on the periodic table are arranged...

a)

Vertically

b)

Horizontally

c)

Diagonally from bottom right corner

d)

Diagonally from top right corner

20.

Which accurately describes nonmetals?

a)

Poor conductors of electricity

b)

Often used in computer parts

c)

Both malleable and ductile

d)

Both dull and brittle

21.

Which group on the periodic table is the most reactive?

a)

Group 1

b)

Group 2

c)

Group 13

d)

Group 18

22.

How many periods are there in the periodic table?

a)

7

b)

9

c)

10

d)

18

23.

Identify the unknown atom.

a)

Flourine

b)

Beryllium

c)

Boron

d)

Helium

24.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
25.

The yellow elements in this table are called

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

26.
Which of the following is not a property of metals?
a)
brittle
b)
malleable
c)
lustrous
d)
conductive
27.
Good conductor of heat
a)
Metal
b)
Nonmetal
28.
If a material can easily be drawn into the shape of a wire, it is
a)
Ductile
b)
Magnetic
c)
Malleable
d)
Reactive
29.

What did Mendeleev notice about the elements that led to his organization of the periodic table?

a)

elements had repeating patterns of properties

b)

elements had increasing numbers of protons

c)

elements had increasing numbers of electrons

d)

elements could be made in a lab

30.
Which part of the atom is responsible for chemical bonding?
a)
Inner/Core Electrons
b)
Outer/Valence Electrons
c)
Protons
d)
Neutrons
31.
What best describes valence electrons?
a)
Electrons in the inner-most shell.
b)
Electrons in the outer-most shell.
c)
Electron that became a beta particle.
32.
Where are valence electrons located?
a)
In the inner-most shell of an atom.
b)
In the outer-most shell of an atom.
c)
Between the inner and outer shells of an atom.
d)
Inside the nucleus of an atom.
33.
How many valence electrons do most atoms need to have a complete outer shell and be happy?
a)
1
b)
8
c)
10
d)
5
34.
Which two elements only need two valence electrons to be happy?
a)
Hydrogen and Helium
b)
Lithium and Neon
c)
Copper and Iron
d)
Californium and Berkelium
35.
Why do Hydrogen and Helium only need two valence electrons?
a)
The first electron shell can only hold two electrons.
b)
They are both metals.
c)
They both begin with H.
d)
They are both gases.
36.
How many valence electrons do elements in Group 1, the Alkali Metals, have?
a)
1
b)
2
c)
6
d)
7
37.
How many valence electrons do elements in Group 2, the Alkaline Earth Metals, have?
a)
1
b)
2
c)
6
d)
7
38.
How do ions form?
a)
Atoms gain or lose electrons to fill or empty the valence shell.
b)
Atoms like cats so they become "pawww-sitive".
c)
Atoms gain or lose electrons to change their atomic mass.
d)
Atoms gain or lose electrons to match the number of neutrons.
39.
If an element gives away an electron, will it form a positive ion or a negative ion?
a)
Positive.
b)
Pawww-sitive.
c)
Negative.
d)
Neutral.
40.
If an element gains an electron, will it form a positive ion or a negative ion?
a)
Positive.
b)
Negative.
c)
Neutral.
d)
Square root of -1.
41.
Why does an ion have a charge?
a)
There are different numbers of protons and neutrons.
b)
There are different numbers of neutrons and electrons.
c)
There are different numbers of protons and electrons.
d)
There are different numbers for atomic mass and atomic number.
42.
How do ionic bonds form?
a)
Atoms share electrons to fill their valence shell.
b)
Atoms gain or lose electrons to fill their valence shell.
c)
Atoms donate electrons to a "sea" of electrons.
43.
How do covalent bonds form?
a)
Atoms share electrons to fill their valence shell.
b)
Atoms gain or lose electrons to fill their valence shell.
c)
Atoms donate electrons to a "sea" of electrons.
44.

What is the difference between ionic and covalent bonding?

a)

Ionic bonding involves the transfer of electrons, while covalent bonding involves the sharing of electrons.

b)

Ionic bonding occurs between two nonmetals, while covalent bonding occurs between a metal and a nonmetal.

c)

Ionic bonding involves the sharing of electrons, while covalent bonding involves the transfer of electrons.

d)

Ionic bonding results in the formation of a molecule, while covalent bonding results in the formation of a crystal lattice.

45.

Which type of bonding involves the transfer of electrons?

a)

Ionic bonding

b)

Hydrogen bonding

c)

Metallic bonding

d)

Covalent bonding

46.

In an ionic bond, which type of atoms tend to lose electrons?

a)

metal atoms

b)

Transition metal atoms

c)

Noble gas atoms

d)

Non-metal atoms

47.

Harper, Aria, and Isla are studying chemistry together. They are discussing about covalent bonds. Harper asks, 'How many electrons are typically shared in a single covalent bond?'

a)

2

b)

3

c)

4

d)

1

48.

What is the charge of an ion formed in an ionic bond?

a)

Positive or negative

b)

Neutral

c)

Zero

d)

Opposite

49.

What is the octet rule?

a)

Atoms tend to gain, lose, or share electrons to achieve a full inner shell of eight electrons.

b)

Atoms tend to gain, lose, or share electrons to achieve a full outer shell of six electrons.

c)

Atoms tend to gain, lose, or share electrons to achieve a full outer shell of ten electrons.

d)

Atoms tend to gain, lose, or share electrons to achieve a full outer shell of eight electrons.

50.

Give an example of a compound formed by ionic bonding.

a)

potassium bromide (KBr)

b)

carbon dioxide (CO2)

c)

sodium chloride (NaCl)

d)

magnesium sulfate (MgSO4)

51.
The bond between Na & F.   Ionic or covalent?
a)
Ionic
b)
Covalent
52.
The bond between N & H.   Ionic or covalent?
a)
Ionic
b)
Covalent
53.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
54.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
55.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
56.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
57.

In which type of reaction does a single element replace another element in a compound?

a)

Displacement reaction

b)
Combustion reaction
c)
Decomposition reaction
d)

Double Displacement reaction

58.

Which of the following is an example of a double displacement reaction?

a)

The reaction between hydrochloric acid and sulfuric acid

b)

The reaction between iron (III) oxide and carbon monoxide

c)

The reaction between potassium hydroxide and nitric acid

d)

The reaction between silver nitrate and sodium chloride

59.

Which reaction type often involves a metal reacting with an acid to produce hydrogen gas?

a)
Decomposition reaction
b)
Single displacement reaction
c)
Combustion reaction
d)
Double displacement reaction
60.

What type of reaction occurs when iron reacts with oxygen to form iron(III) oxide?

a)
Combustion reaction
b)

Combination reaction

c)
Decomposition reaction
d)
Acid-base reaction
61.

Which characteristic is common to both displacement and double displacement reactions?

a)
Release of energy
b)
Exchange of ions
c)
Change in color
d)
Formation of a gas
62.

Identify this type of reaction:

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

63.

Which of the following is an example of a synthesis reaction?

a)

2H2O → 2H2 + O2

b)

Na + Cl2 → 2NaCl

c)

CaCO3 → CaO + CO2

d)

H2 + Cl2 → 2HCl

64.

What type of reaction is represented by the equation: 2K + 2H2O → 2KOH + H2?

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

65.

In the chemical equation, H2O2 --> H2O + O2, the H2O2 is a _____.

a)

Product

b)

Reactant

66.

This reaction represents: FeS + HCl ---> FeCl2 + H2S

a)

Synthesis Reaction

b)

Decomposition Reactions

c)

Single Displacement Reaction

d)

Double Displacement Reaction

67.

This type of reaction: Zn+ 2HCl → ZnCl2 + H2

a)

Synthesis Reaction

b)

Decomposition Reaction

c)

Single Displacement Reaction

d)

Double Displacement Reaction

68.

This reaction: 2Al2O3 —> 4Al + 3O2

a)

Synthesis Reaction

b)

Decomposition Reaction

c)

Single Displacement Reaction

d)

Double Displacement Reaction

69.
Pb + FeSO4 ----> PbSO4 + Fe
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
70.
Na3PO4 + 3 KOH ----> 3 NaOH + K3PO4
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
71.
In a chemical reaction, everything to the right of the arrow is called ______________.
a)
Products
b)
Yields
c)
Molecules
d)
Reactants
72.

Which of the following is a compound?

a)

zinc (Zn)

b)

magnesium (Mg)

c)

sodium chloride (NaCl)

d)

potassium (K)

73.

Which of the following is an element?

a)

potassium chloride (KCl)

b)

water (H2O)

c)

carbon (C)

d)

calcium carbonate (CaCO3)

74.

In the equation,  2Mg + O2 ---> 2MgO, which substance(s) are the reactants?

a)
Mg and O
b)
MgO
c)
Mg and MgO
d)
O and MgO
75.

In the reaction above water is a ________________.

a)

Reactant

b)

Product

76.

The reactants in the image above are:

a)

CH4 and 2 O2

b)

2 H2O and CO2

c)

All of these are reactants

d)

All of these are products

77.
Evidence of a chemical reactions is anything that shows - 
a)
a new substance has formed
b)
a solid dissolved in a liquid
c)
interaction between 2 gases
d)
a change in the state of matter
78.

How many elements are in this chemical formula?

H2SO4H_2SO_4  

a)

1

b)

2

c)

3

d)

4

79.

What elements are represented in this chemical formula? Fe2O3 

a)

Iron, Oxygen

b)

Francium, Europium, Oxygen

c)

Ferrium, Oxygen

d)

Berylium, Oxygen

80.

What is the total number of atoms in this formula? H2O2H_2O_2  

a)

2

b)

4

c)

3

81.

Which of the following elements is least likely to form a compound?

a)

Hydrogen

b)

Sodium

c)

Argon

d)

Potassium

82.

Is this an element or a compound? CaSO4CaSO_4  

a)

Element

b)

Compound

83.

In a chemical reaction, everything to the left of the arrow is called ______________.

a)

Reactants

b)

Products

c)

Compounds

d)

Precipitates

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