Chemistry Chapter 9 Test Review

Front 1

Network Solid

Back 1

a solid in which all of the atoms are covalently bonded to each other

Front 2

Resonance structures

Back 2

(can be reversed/ reversely drawn)
-are structures that occur when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion.

Front 3

Dispersion forces

Back 3

between non polar forces (like Carbon Tetra Chloride CCl4) the molecule doesn’t have a pole but it has a temporary charge after moving around all the time there will be a moment in time in that moment it will have a partially negative charge

Front 4

Molecular Formula

Back 4

An expression which states the number and type of atoms present in a molecule of a substance.
like C6H14

Front 5

Structural Formula

Back 5

a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion

Front 6

Triple Covalent Bond

Back 6

a bond formed by sharing three pairs of electrons
one is sigma
the other two are pi

Front 7

Dispersion Force

Back 7

attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules

Front 8

Double Covalent Bond

Back 8

a bond that involves two shared pairs of electrons
one is a sigma bond and the other is a pi bond

Front 9

Coordinate Covalent Bond

Back 9

a covalent bond in which one atom contributes both bonding electrons

Front 10

Non Polar Covalent Bond

Back 10

a covalent bond in which the electrons are shared equally by the two atoms

Front 11

A dipole
Dipole forces

Back 11

-a molecule that has two poles, or regions with opposite charges
-intermolecular forces resulting from the attraction of oppositely charged regions of polar molecules

Front 12

dipole interactions

Dipole interactions are similar & weaker than...

Back 12

The attractions between opposite poles of polar molecules
di (two) poles
dipole
-ionic bonds

Front 13

bond dissociation energy

Back 13

the amount of energy required to break a covalent bond between atoms

Front 14

VSEPR theory

Back 14

states that because electron pairs repel, molecules adjust their shapes so that valence-electron pairs are as far apart as possible

Front 15

Hydrogen bonds can create very strong intermolecular forces when they are bonded to atoms that are very electronegative like...

Back 15

oxygen, nitrogen, and flourine

Front 16

When LIKE atoms are joined by a covalent bond, the bonding electrons are shared equally and the bond is...

Back 16

non polar covalent

Front 17

In general, the electronegativity values of nonmetallic elements are greater than the electronegativity values of...

Back 17

metallic elements

Front 18

A polar molecule
polar covalent bond (polar bond)

Back 18

-a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive
-a covalent bond between atoms in which the electrons are shared unequally

Front 19

Hydrogen bonds

Back 19

attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom

Front 20

Describe a network solid and give two examples

Back 20

Solids that consist of molecules that very stable and tend to not melt until the temperature reaches 1000*c or higher are known as network solids or network crystals. Network solids contain atoms that are all covalently bonded to each other. The only way a network solid can be melted is if all of the covalent bonds must be broken throughout the solid, but even then, the solid wont melt. Like diamond, rather than melting, it vaporizes into a gass at 3400*C and above rather.

C (diamond)-a form of pure carbon-
SiO2 (quartz)-silicon dioxide- the solid is an extended three-dimensional network of ...-Si-O-Si-O-... bonding.

Diamond is a network solid consisting of carbons that are interconnecting and covalently bonded throughout the molecule. Quartz is another example of a network solid. Quartz or silicon dioxide (SiO2) is a stone (like diamond) that is composed of an extended 3 dimensional network of …Si-O-Si-O… bonding.