WorksheetsAS-Chemistry Worksheet: Definitions, basic maths skills (Sep 26)
Total questions: 49
Worksheet time: 25mins
An atom is defined as:
A form of energy.
The smallest unit of matter that retains the properties of an element.
A type of chemical reaction.
A large molecule made up of many elements.
An element is defined as which of the following?
A mixture of two or more substances.
A substance that can be separated by physical means.
A compound made of different atoms.
A substance that cannot be broken down into simpler substances by chemical means.
A compound is defined as:
A mixture of two or more substances that are not chemically combined.
A substance made up of two or more different elements chemically combined.
A single element in its purest form.
A solution of solids dissolved in a liquid.
An ion is defined as:
A neutral atom with no charge.
An atom or molecule with a net electric charge due to the loss or gain of one or more electrons.
A molecule that cannot conduct electricity.
A particle with only protons and neutrons.
A molecule is defined as:
A single atom with no bonds.
A group of two or more atoms bonded together.
A type of chemical reaction.
A charged particle formed by loss or gain of electrons.
An isotope is defined as:
Atoms of different elements with the same number of protons.
Atoms of the same element with different numbers of neutrons.
Atoms of the same element with different numbers of protons.
Atoms of different elements with the same number of electrons.
Exothermic is defined as:
A process that absorbs heat energy from its surroundings.
A process that does not involve any energy change.
A process that only occurs at low temperatures.
A process that releases heat energy to its surroundings.
The atomic number is defined as:
The number of neutrons in the nucleus of an atom.
The number of protons in the nucleus of an atom.
The total number of electrons and protons in an atom.
The mass number of an atom.
The definition of Empirical formula is:
The actual number of atoms of each element in a molecule.
The simplest whole-number ratio of atoms of each element in a compound.
The total mass of a compound divided by its molar mass.
The arrangement of atoms in a crystal lattice.
What is the symbol for Hydrogen?
O
He
H
N
What is the symbol for Sodium?
Sn
So
Sd
Na
What is the symbol for Argon?
Ag
Au
Al
Ar
What is the symbol for Mercury?
Me
Hg
Mc
Mr
What is the symbol for Gold?
Ag
Fe
Cu
Au
What is the symbol for Lead?
Le
Pb
Ld
La
What is the symbol for Cobalt?
Ct
Co
Cu
Cb
What is the symbol for Manganese?
Mg
Mo
Ma
Mn
What is the symbol for Seaborgium?
Sb
Sg
Sr
Sm
What is the formula for Water?
CO2
NaCl
O2
H2O
What is the formula for Ammonia?
NH4
NO2
NH3
N2H4
What is the formula for Methane?
CO2
CH4
C2H6
CH3OH
What is the formula for Sulphuric acid?
HCl
HNO3
H2SO4
H2CO3
What is the formula for HCl?
Sulfuric acid
Hydrochloric acid
Nitric acid
Acetic acid
What is the formula for CaCO3?
Calcium chloride
Calcium carbonate
Calcium sulfate
Calcium oxide
What is the formula for Mg(OH)2?
Magnesium oxide
Magnesium carbonate
Magnesium sulfate
Magnesium hydroxide
What is the formula for C2H4?
Methane
Ethene
Propane
Butane
What is the formula for Al(SO4)3?
Aluminium phosphate
Aluminium sulfate
Aluminium sulfide
Aluminium nitrate
What is the relative charge of a Proton?
-1
+1
0
+2
What is the relative mass of a Proton?
0.0005
1
0.5
2
Complete the following table: Where is a Proton found?
Cytoplasm
Nucleus
Cell membrane
Mitochondria
What is the relative charge of a Neutron?
+1
0
-1
+2
What is the relative mass of a Neutron?
0.0005
1
0.5
2
Complete the following table: Where is a Neutron found?
Cytoplasm
Nucleus
Cell membrane
Mitochondria
Fill in the blank: The subatomic particle with a negative charge is called an ________.
proton
neutron
positron
electron
Balance the following equation: C + O₂ → CO
C + O₂ → CO₂
2C + O₂ → 2CO
C₂ + O₂ → 2CO
C + 2O₂ → CO₂
Balance the following equation: N₂ + H₂ → NH₃
N₂ + 2H₂ → 2NH₃
N₂ + 3H₂ → 2NH₃
N₂ + H₂ → NH₃
N₂ + 3H₂ → NH₃
Balance the following equation: C₂H₄ + O₂ → H₂O + CO₂
C₂H₄ + 2O₂ → 2H₂O + CO₂
C₂H₄ + O₂ → H₂O + CO₂
C₂H₄ + 3O₂ → 2H₂O + 2CO₂
C₂H₄ + 4O₂ → 2H₂O + 2CO₂
Write the following numbers in standard form. b) 34500
3.45x103
34.5 x 10^3
0.345 x 10^5
3.45x104
For each of the numbers in questions 1–6, state the number of significant figures and the number of decimal places. 5. 560.0
Significant figures: 3, Decimal places: 1
Significant figures: 4, Decimal places: 1
Significant figures: 4, Decimal places: 0
Significant figures: 3, Decimal places: 0
For each of the numbers in questions 1–6, state the number of significant figures and the number of decimal places. 6. 0.000480
Significant figures: 3, Decimal places: 6
Significant figures: 2, Decimal places: 5
Significant figures: 4, Decimal places: 3
Significant figures: 3, Decimal places: 5
Rearrange the following equations to give the letter shown as the subject. a) What does c equal if q = mcT ?
c = m / (qT)
c = q / (mT)
c = T / (qm)
c = qT / m
What does T equal if G = H - TS?
T = (G - H)/S
T = (H + G)/S
T = (H - G)/S
T = (G + H)/S
Simplify the following ratio: 56:88
8:13
7:11
14:19
4:7
There are 100 balls in a bag. The balls are red, blue, green or white. The ratio of blue to red is 5:1. There are twice as many blue as green. 1/4 of the balls are green. How many white balls are in the bag?
10 white balls
15 white balls
25 white balls
20 white balls
Determine the units of density given that density = mass (g) / volume (cm³).
cm³/g
g/cm
g·cm³
g/cm³
Determine the units of concentration given that concentration = number of moles (mol) / volume (dm³).
dm³/mol
mol/dm³
mol·dm³
mol+dm³
Pharmacists often calculate the concentration of substances for dosages. In this case the volumes are smaller, measured in cm³, and the amount is given as a mass in grams. Determine the units of concentration when concentration = mass(g) / volume(cm³).
mg/cm³
g/L
cm³/g
g/cm³
Rate of reaction is defined as the ‘change in concentration per unit time’. Determine the units for rate when concentration is measured in mol dm⁻³ and time in seconds.
mol s⁻¹
mol dm⁻³ s⁻¹
dm⁻³ s⁻¹
mol dm³ s⁻¹
Use the formula pressure = force / area to determine the SI unit of pressure that is equivalent to the Pascal.
kg/m³
J/s
N/m²
W/m²
