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WorksheetsAQA Trilogy Chemistry Paper 1 Basics (1 of 2)
Total questions: 35
Worksheet time: 18mins
Name
Class
Date
1.
What are the 3 sub-atomic particles called?
a)
potions, neutrons and electrons
b)
protons, neurons and electrons
c)
protons, neutrons and elections
d)
protons, neutrons and electrons
2.
What is the mass number?
a)
Number of protons plus neutrons
b)
Number of protons plus electrons
c)
Number of neutrons plus electrons
3.
What is the atomic number?
a)
Number of protons plus electrons
b)
Number of protons
c)
Number of protons plus neutrons
d)
Number of protons, neutrons and electrons
4.
What is the charge on a proton?
a)
positive 1
b)
0
c)
negative 1
5.
What is the charge on a neutron?
a)
positive 1
b)
0
c)
negative 1
6.
What is the charge on an electron?
a)
positive 1
b)
0
c)
negative 1
7.
How many protons, neutrons and electrons does a lithium atom have?
a)
p=3 n=4 e=3
b)
p=3 n=7 e=3
c)
p=3 n=4 e=4
8.
Where are the protons and neutrons found?
a)
In isotopes
b)
In ions
c)
In the nucleus
d)
In shells
9.
Where are the electrons found?
a)
In isotopes
b)
In ions
c)
In the nucleus
d)
In shells
10.
How mant electrons fill each shell?
a)
2, 4, 6....
b)
2, 4, 8....
c)
8, 8, 8....
d)
2, 8, 8....
11.
An isotope is an atom with the same number of....
a)
protons and neutrons but a different number of electrons.
b)
neutrons and electrons but a different number of protons.
c)
protons and electrons but a different number of neutrons.
12.
In what order are elements on the modern periodic table?
a)
Mass number
b)
Atomic Mass
c)
Atomic number
d)
Relative Atomic Mass
13.
Which is NOT a property of metals.
a)
good electrical conductor
b)
good electrical insulator
c)
good thermal conductor
d)
high melting & boiling point
14.
Which is NOT a property of non-metals?
a)
low density
b)
good electrical conductor
c)
brittle
d)
good thermal insulator
15.
How did Mendeleev arrange the periodic table?
a)
Grouped elements with similar properties. Left gaps for undiscovered elements.
b)
Grouped elements with different properties. Left gaps for undiscovered elements.
16.
Lithium + water ->
a)
lithium oxide + hydrogen
b)
lithium hydroxide + water
c)
lithium hydroxide + hydrogen
17.
What would you NOT see if potassium reacted with water?
a)
Metal would sink
b)
Metal moves along surface of water
c)
Lilac flame
d)
Fizzing
18.
Sodium chloride + fluorine -->
a)
Sodium chloride + fluorine
b)
Sodium + chlorine
c)
Sodium fluoride + chlorine
19.
Why are Group 0/Noble gases unreactive?
a)
They are gases
b)
Full outer shell of electrons
c)
Too many protons
20.
Why is fluorine more reactive than bromine?
a)
Fluorine has less shells so attraction between nucleus and outer electrons is stronger
b)
Fluorine has more shells so attraction between nucleus and outer electrons is stronger
21.
Why is potassium more reactive than sodium?
a)
Potassium has more shells so attraction between nucleus and outer electrons is stronger
b)
Potassium has more shells so attraction between nucleus and outer electrons is weaker
22.
From which alkali metal is it easiest to remove the outer electron?
a)
Li
b)
Na
c)
K
23.
Which halogen is it easiest to give an outer electron?
a)
F
b)
Cl
c)
Br
24.
What type of structure & bonding is in H2O?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
25.
What type of bonding is in graphine?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
26.
What type of bonding is in magnesium chloride?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
27.
What type of bonding is in calcium?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
28.
What type of bonding is in sodium chloride?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
29.
What type of bonding is in silicon dioxide?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
30.
Why are alloys harder than pure metals?
a)
Distorted structure. Layers can not slide.
b)
Distorted structure. Layers can slide.
31.
Why does sodium chloride have a high melting point?
a)
Lots of energy needed to break the strong electrostatic forces between positive metal ions and electrons.
b)
Lots of energy needed to break the strong electrostatic forces between oppositely charged ions.
32.
Why can ionic compounds only conduct electricity when molten or in a solution?
a)
Ions are free to move so can carry charge through the structure.
b)
Electrons are free to move so can carry charge through the structure.
33.
Why is methane a gas at room temperature?
a)
Weak intermolecular forces between molecules, so little energy needed to break.
b)
Weak bonds, so little energy needed to break.
34.
Why is diamond hard?
a)
4 strong covalent bonds between carbons.
b)
4 weak covalent bonds between carbons.
35.
Why does anything conduct electricity?
a)
Charged particles can move
b)
Charged particles can flow throughout the structure
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