Ionisation Energy & Electromagnetic Spectrum

Mass and charge of a proton

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

Relative mass and charge of an electron

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

Subatomic particles in the nucleus

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

Atoms are made of subatomic particles

True.

Electrons have a larger mass than protons

False. Electrons have a much smaller mass than protons.

Sub-atomic particle not found inside the nucleus

The sub-atomic particle that is not found inside the nucleus is the electron.

Relative mass and charge of a neutron

A neutron has a relative mass of 1 and charge of 0.

Nucleus of an atom charge

False. The nucleus of an atom has a positive charge due to the presence of positive protons and neutral neutrons.

Subatomic particles in the nucleus

The subatomic particles in the nucleus are known as nucleons.

Mass of an atom concentration

The mass of an atom is concentrated in the nucleus.

Define atomic number

Atomic number is the number of protons.

Define mass number

Mass number is the number of protons and neutrons.

Calculate number of neutrons in an atom

Number of neutrons = mass number - atomic number OR Number of neutrons = mass number - number of protons.

Determine number of electrons in an atom

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

Protons, neutrons, and electrons in Al

The number of protons, neutrons and electrons in an atom of Al₁₃²⁷ are: Protons = 13, Neutrons = 27 - 13 = 14, Electrons = 13.

Atoms and ions of the same element

True. Atoms and ions of the same element have the same number of protons.

Symbol for atomic mass

False. The symbol used to represent atomic mass is A.

Why are atoms electrically neutral?

Atoms are electronically neutral because they have the same number of protons and electrons so the positive and negative charges cancel each other out.

Protons, neutrons, and electrons in Mg2+

The number of protons, neutrons and electrons in a magnesium ion, Mg²⁺ is: Protons = 12, Neutrons = 12, Electrons = 10.

Symbol for atomic number

The symbol used to represent atomic number is Z.

Protons, neutrons, and electrons in O2-

The number of protons, neutrons and electrons in a chloride ion, O²⁻ is: Protons = 8, Neutrons = 8, Electrons = 10.

What is an isotope?

An isotope is an atom of the same element containing the same number of protons but different numbers of neutrons.

Isotopes example

The isotopes are C₆¹³ and C₆¹⁴.

Information to calculate relative atomic mass

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

Equation for Ar

State the equation for Ar in terms of the percentage abundance and mass of isotopes A and B.

Relative Atomic Mass Equation

The equation for calculating relative atomic mass in terms of the percentage abundance and mass of isotopes A and B is: ( (percent of isotope A x mass of isotope A) + (percent of isotope B x mass of isotope B) ) / 100.

Relative Atomic Mass Calculation

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

Isotope Abundance

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

Relative Atomic Mass Method

Relative atomic mass is calculated by multiplying the abundance of each isotope by its mass, adding these numbers together, and then dividing this value by the total abundance.

Isotope Identification

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

Identifying Elements

After calculating the Ar, you would identify an element by looking for the value on the Periodic Table.

Example of Ar Calculation

For example, Ar = 23. On the Periodic Table, the element with an Ar of 23 is sodium.

Relative Atomic Mass Calculation Example

The relative atomic mass of the element is: (71 x 39) + (69 x 61) / 100 = 69.8 or 70.

Isotope Chemical Characteristics

Isotopes display the same chemical characteristics.

Chemical Characteristics Determinant

The chemical characteristics of an atom are determined by the number of electrons in the outer shell.

Mass Spectra Purpose

Mass spectra is used to determine the relative atomic mass of an element from its isotopes.

Relative Atomic Mass Range

The element has a relative atomic mass between 70 and 71 because there is a greater abundance of the isotope with a mass of 70 than 72.

Mass Spectrum Calculation

The relative atomic mass of the element is: (121 x 57.2) + (123 x 42.8) / 100 = 121.9.

Boron Relative Atomic Mass

The relative atomic mass of boron is: (19.9 x 10) + (80.1 x 11) / 100 = 10.8.

Isotopes in Sample

There are three isotopes present in this sample as there are three peaks.