Chemistry Revision - ATOMIC STRUCTURE REVIEW TOPIC 2

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ATOMIC STRUCTURE REVIEW – TOPIC 2

State the position of the subatomic particles, their relative masses and charges.

Protons: 1 atomic mass unit & + charge

Neutrons: 1 atomic mass unit & 0 charge

Electrons: 1/1836 atomic mass unit & - charge

Define the terms of mass number [A] and atomic number [Z] and be able to identify isotopes and ions of elements.

AZE Notation: The number at the top left represents the mass number and the bottom left the atomic number

Mass Number: The total number of protons and neutrons in a nucleus

Atomic Number: The number of protons in the nucleus of an atom, which determines the chemical properties of an element and its place in the periodic table.

EXAMPLE: 56 Fe 26 –

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The mass number = protons + neutrons = 56

The atomic number = number of protons = 26

Therefore the number of neutrons = 56-26 = 30

Isotopes are atoms of the same element with different mass numbers (atoms of the same element must contain the same number of protons, but can contain a different number of neutrons)

Be able to identify protons, neutrons and electrons in isotopes and in ions.

For a given element the number of protons never changes

The number of neutrons depends on the mass number of the isotope in question

The number of electrons ...

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