What is the mass and charge of a proton ?

A proton has a relative mass of 1 and a charge of +1.

True or False? All atoms of the same element have the same number of protons.

True . All atoms of the same element have the same number of protons.

What is the mass and charge of an electron ?

An electron has a negligible mass and a charge of -1.

Define atomic number .

Atomic number is the number of protons in the nucleus of an atom.

What information does the mass number give?

The mass number is the total number of protons and neutrons in the nucleus of an atom.

An isotope is an atom of the same element with: A different number of neutrons and hence, a different mass number. The same number of protons (and electrons).

Which subatomic particles are in the nucleus of an atom?

The subatomic particles in the nucleus of an atom are protons and neutrons.

How do you calculate the number of neutrons in an atom?

To calculate the number of neutrons in an atom: Number of neutrons = mass number - atomic number OR Number of neutrons = mass number - number of protons

A molecule is a group of two or more atoms held together by chemical bonds.

True or False? Atoms are made of subatomic particles.

True . Atoms are made of subatomic particles including protons, neutrons, and electrons.

Define relative atomic mass .

Relative atomic mass is: The ratio of the average mass of atoms of an element to 1/12 of the mass of an atom of carbon-12 OR The average mass of an atom compared to 1/12 of the mass of an atom of carbon-12

Which subatomic particle has a mass of 1 and a charge of 0?

The subatomic particle with a mass of 1 and a charge of 0 is the neutron.

How do you determine the number of electrons in an atom?

The number of electrons in an atom is the same as the number of protons / the atomic number.

State two pieces of information required to calculate the relative atomic mass of an element.

Two pieces of information required to calculate the relative atomic mass of an element are: The mass numbers of each isotope. The (relative / percentage) abundances of each isotope.

True or False? The relative atomic mass of an element can be calculated using the atomic numbers and relative abundances of all its isotopes.

False . The relative atomic mass of an element is calculated using the mass numbers and relative abundances of all its isotopes.

In terms of isotopes , what is abundance?

In terms of isotopes, abundance is the amount of each isotope present in a sample of an element.

True or False? Relative atomic mass is calculated by adding the mass numbers of all isotopes.

False . Relative atomic mass is calculated by: Multiplying the abundance of each isotope by its mass Adding these numbers together Then, dividing this value by the total abundance.

How can you recognise isotopes from their chemical symbol?

Isotopes have the same symbol and same atomic numbers but different mass numbers.

After calculating the A r , how would you identify an element?

After calculating the A r , you would identify an element by looking for the value on the Periodic Table. For example, A r = 23. On the Periodic Table, the element with an A r of 23 is sodium.

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What is the mass and charge of a proton?

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What is the mass and charge of a proton?
A proton has a relative mass of 1 and a charge of +1.
True or False?
All atoms of the same element have the same number of protons.
True.
All atoms of the same element have the same number of protons.
What is the mass and charge of an electron?
An electron has a negligible mass and a charge of -1.
Define atomic number.
Atomic number is the number of protons in the nucleus of an atom.
What information does the mass number give?
The mass number is the total number of protons and neutrons in the nucleus of an atom.
What is an isotope?
An isotope is an atom of the same element with:
- A different number of neutrons and hence, a different mass number.
- The same number of protons (and electrons).
Which subatomic particles are in the nucleus of an atom?
The subatomic particles in the nucleus of an atom are protons and neutrons.
How do you calculate the number of neutrons in an atom?
To calculate the number of neutrons in an atom:
- Number of neutrons = mass number - atomic number
  OR
- Number of neutrons = mass number - number of protons
What is a molecule?
A molecule is a group of two or more atoms held together by chemical bonds.
True or False?
Atoms are made of subatomic particles.
True.
Atoms are made of subatomic particles including protons, neutrons, and electrons.
Define relative atomic mass.
Relative atomic mass is:
- The ratio of the average mass of atoms of an element to 1/12 of the mass of an atom of carbon-12
  OR
- The average mass of an atom compared to 1/12 of the mass of an atom of carbon-12
Which subatomic particle has a mass of 1 and a charge of 0?
The subatomic particle with a mass of 1 and a charge of 0 is the neutron.
How do you determine the number of electrons in an atom?
The number of electrons in an atom is the same as the number of protons / the atomic number.
Calculate the number of protons, neutrons and electrons in an atom of ${}_{13}^{27}{Al}$ .
The number of protons, neutrons and electrons in an atom of ${}_{13}^{27}{Al}$ are:
- Protons = 13
- Neutrons = 27 - 13 = 14
- Electrons = 13
State two pieces of information required to calculate the relative atomic mass of an element.
Two pieces of information required to calculate the relative atomic mass of an element are:
- The mass numbers of each isotope.
- The (relative / percentage) abundances of each isotope.
State the equation for A_r in terms of the percentage abundance and mass of isotopes A and B.
The equation for calculating relative atomic mass in terms of the percentage abundance and mass of isotopes A and B is:
$\frac{(% of isotope A \times mass of isotope A) + (% of isotope B \times mass of isotope B)}{100}$
True or False?
The relative atomic mass of an element can be calculated using the atomic numbers and relative abundances of all its isotopes.
False.
The relative atomic mass of an element is calculated using the mass numbers and relative abundances of all its isotopes.
In terms of isotopes, what is abundance?
In terms of isotopes, abundance is the amount of each isotope present in a sample of an element.
Which of the following are isotopes?
${}_{6}^{13}C$ ${}_{6}^{14}C$ ${}_{7}^{14}N$
The isotopes are ${}_{6}^{13}C$ and ${}_{6}^{14}C$ .
${}_{7}^{14}N$ is not an isotope because it is a different element (nitrogen not carbon).
True or False?
Relative atomic mass is calculated by adding the mass numbers of all isotopes.
False.
Relative atomic mass is calculated by:
- Multiplying the abundance of each isotope by its mass
- Adding these numbers together
- Then, dividing this value by the total abundance.
How can you recognise isotopes from their chemical symbol?
Isotopes have the same symbol and same atomic numbers but different mass numbers.
After calculating the A_r, how would you identify an element?
After calculating the A_r, you would identify an element by looking for the value on the Periodic Table.
For example, A_r = 23. On the Periodic Table, the element with an A_r of 23 is sodium.
Calculate the relative atomic mass of an element using this information about its isotopes:
- Isotope 1: Mass = 71, abundance = 39%
- Isotope 2: Mass = 69, abundance = 61%
The relative atomic mass of the element is:
$\frac{(71 \times 39) + (69 \times 61)}{100}$ = 69.8 or 70

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Atomic Structure (Edexcel IGCSE Chemistry)

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Cards in this collection (23)

1. Principles of Chemistry

States of Matter

Elements, Compounds & Mixtures

Atomic Structure

The Periodic Table

Chemical Formulae, Equations, Calculations

Ionic Bonding

Covalent Bonding

Metallic Bonding

Electrolysis

2. Inorganic Chemistry

Group 1 (Alkali Metals)

Group 7 (Halogens)

Gases in the Atmosphere

Reactivity Series

Extraction & Uses of Metals

Acids, Alkalis & Titrations

Acids, Bases & Salt Preparations

Chemical Tests

3. Physical Chemistry

Energetics

Rates of Reaction

Reversible Reactions & Equilibria

4. Organic Chemistry

Introduction

Crude Oil

Alkanes

Alkenes

Alcohols

Carboxylic acids

Esters

Synthetic polymers