Atomic Basics
This is the smallest unit that still keeps the properties of an element.
The atom
An atom that gains electrons becomes this type of ion.
An anion
The maximum number of electrons in a p orbital.
6
Group 1 elements are known by this name.
Alkali metals
Metals become more reactive in this direction on the periodic table.
down and to the left
This part of the atom contains most of its mass.
The nucleus
An atom that loses electrons becomes this type of ion.
A cation
The number of electrons in a neutral carbon atom
6
Group 18 elements are called this because they rarely react.
Noble gases
Nonmetals become more reactive in this direction.
Up and to the right
Atoms of the same element with different numbers of neutrons are called this.
Isotopes
How you calculate the charge of an atom.
protons minus electrons
The number of valence electrons in carbon
4
Group 17 elements are known for being very reactive nonmetals.
Halogens
This trend describes how strongly an atom pulls on electrons in a bond.
electronegativity
The number that tells you how many protons an atom has
Atomic number
An atom with more electrons than protons will have this type of charge.
Negative
This notation shows how electrons are arranged in orbitals (1s² 2s²...).
electron configuration
Elements in groups 3–12 are called this.
Transition metals
Elements in the same column share this characteristic.
similar properties (or same number of valence electrons)
This equals the total number of protons plus neutrons in an atom.
Mass number
Why potassium typically forms a +1 ion
It loses one valence electron
Why electrons fill lower energy levels first.
to achieve the most stable (lowest energy) arrangement
Group 2 elements are known as this family.
alkaline earth metals
This trend generally increases across a period from left to right.
Electronegativity