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Chapter 6 - Chemical Bonds Study Guide
Terms in this set (36)
the force that holds cations and anions together
a chemical bond in which atoms share a pair of valence electrons.
An atom that has a net positive or negative charge.
an ion with a negative charge.
an ion with a positive charge.
a mixture of two or more elements, at least one of which is a metal.
A process that involves rearrangement of the molecular or ionic structure of a substance,
Polar covalent bond
a covalent bond in which electrons are not shared equally.
Poly atomic Ion
a covalently bonded group of atoms that has a positive or negative charge and acts as a unit.
electron dot diagram
a model of an atom in which each dot represents a valence electron.
solids whose particles are arranged in a lattice structure.
a neutral group of atoms that are joined together by one or more covalent bonds.
when two atoms share one pair of electrons
when two atoms share two pairs of electrons
when two atoms share three pairs of electrons.
the attraction between a metal cation and the shared electrons that surround it.
Energy levels that need to be filled in order to bond
highest energy levels
highest occupied energy level of an atom is filled with electrons
Reason why noble gases are stable
they have the maximum amount of valence electrons.
What an electron dot diagram shows
how many valence electrons an atom has.
This happens to valence electrons in IONIC bonding
they are transferred
Difference between a cation and anion
cation has positive charge
anion has negative charge
what subscripts show in a chemical formula
relative numbers of atoms of the elements present.
type of elements that bond IONICALLY
Metals and nonmetals
type of elements that bond COVALENTLY
2 or more nonmetals
How electrons bond in covalent bonding
two atoms share a pair of valence electrons
charge molecules have
binary ionic compound
a compound made from only two elements
what all anions end in
reason why numerical prefix is used when naming molecular compounds
indicates the number of atoms of each element in the molecule.
two properties of metals
conduct heat and electricity
tend to lose electrons in reactions
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