Chemistry Vocabulary

connect Electronegativity to Covalent Bonding

if the atoms involved have similar electronegativity they will share electrons more or less equally forming a covalent bond.

electronegativity

the atoms ability to attract shared electrons in a chemical bond

covalent bonding

2 atoms share electrons to become a stable electron configuration.

Polar covalent VS. Non-polar covalent

in a polar covalent bond there is a unequal share of electrons due to the atoms having different EN. with a nonpolar covalent bond 2 atoms have similar EN’s causing an equal share of electrons.

polar covalent example

H2O — oxygen is more electronegative than hydrogen

non-polar covalent example

H2 — they are the same atom meaning exact EN’s

VESPR helping Lewis Structures

this theory helps determine the 3D arrangement of atoms in molecules when drawing a Lewis structure

covalent compound

a chemical compound formed by the sharing of electron pairs between non-metals

molecule

2 or more atoms covalently bonded together.

diatomic elements

molecules composed of only 2 atoms, of the same or different chemical elements.

7 naturally occurring diatomic elements

hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine.

VESPR theory

predicts the shape of molecules based on the repulsion between electron pairs. electron pairs will arrange themselves as far apart to minimize repulsion

what constitutes an Electron Domain

bonded pair = electrons shared in a bond

lone pair= electrons not in a bond

multiple bonded pairs = electrons in a double or triple bond

electron domain

the space occupied by electrons

connect chemical bonds, polarity, intermolecular forces, and properties of substances

the type of chemical bond determines the polarity of molecules, which in turn affects the intermolecular forces. these force then influence the physical properties of the substances.

chemical bond

the forces holding the atoms together

polarity

distribution of electrical charge over the atoms

intermolecular forces

the forces of attraction or repulsion between molecules

properties of substances

the type and force of intermolecular forces affect the physical properties of substances

polar molecule example

H2O

Non-polar molecule

CH4 (Methane)

explain how electronegativity can be used to predict Polarity

BEND; Bend is based on bond electronegativity difference which determines if the atom is polar or not

why do polar molecules have the strongest intermolecular forces

polar molecules are a + and - charge, causing an unequal share in electrons, acts as a magnet.

how are noble gases still affects by IMF

still experience intermolecular forces like London dispersion forces due to temporary dipoles caused by electron cloud fluctuations. variations in boiling points among noble gases.

hydrogen bond

hydrogen is bonded to a highly electronegative atom. (strongest IMF)

Dipole - Dipole

the short-range attractive force between polar molecules ( 2nd strongest IMF).

London Dispersion Force (LDF)

occur in all molecules, whether polar or nonpolar. (Weakest IMF)

intermolecular forces related to properties of substance (boiling point and viscosity )

as the IMF strength increases the boiling point of a substance does as well. the stronger the intermolecular forces the higher viscosity levels.

viscosity

a fluids resistance to movement

boiling point

amount of kinetic energy need to overcome the force of attraction

<0.5

nonpolar

0.5 - 2.0

polar

>2.0

ionic

electronegativity increases

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