chem chapter 6

metallic bonded structures

electrons move freely allowing them to be good conductors, malleable, ductile and have luster

unshared pair

pair of electrons that aren’t being used in the bond also called “lone pair”

what are ionic compounds arranged in

a crystal lattice making them stronger

polar covalent bonds

electrons are shared unequally created charged “poles”

nonpolar covalent bonds

electrons are shared equally

central atom

element that occurs the fewest number of times in molecular formula

linear molecule

two electrons, bond angle of 180

triagonal planar

three electrons, bond angle of 120

tetrahedral

four electrons, bond angle of 109.5

chemical bond

mutual attraction between valence electrons in different atoms that binds the atoms together

why do bonds form

to decrease potential energy and create a more stable environment

ionic bond

electrons are given up

covalent bond

electrons are shared

modified tetrahedral

5 or 6 electrons, bond angle of less than 109.5

vser theory

repulsion between the valence electrons in a bond causes the electrons to be placed as far apart as possible

intermolecular forces

attraction between molecules(weak forces)

electronegativity

how strong an atoms attraction is for an electron during the bond

highest electronegativity

flourine(F)

lowest electronegativity

cesium(Cs)

greater than 1.67

ionic

less than 1.67

covalent

characteristics of ionic bonds

conduct electricity, soluble in water, high melting point, compound

characteristics of covalent bonds

nonconductors, insoluble, low melting point, molecule

polar molecule

has a positive and negative side

electron pair repulsion

shared-shared

EPR- weakest

electron pair repulsion

shared-unshared

EPR- middle

electron pair repulsion

unshared-unshared

EPR- strongest

chromotography

how mixtures seperate

dipole-dipole

polar-polar and strongest

London dispersion

nonpolar-nonpolar and weakest and is tempoary

dipole induced dipole

polar-nonpolar(for to be polar) middle

chemical bonding

when electron clouds of atoms overlap

electron affinity

attractoin for an additional electron before bond

do metals want to gain or lose an electron

lose(low electronegativity)

do nonmetals want to gain or lose an electron

gain(high electronegativity)

what are electrostatic forces

what holds an ionic bond together

inter

between 2 molecules

intra

inside 1 molecule

if ions have the same polarity which one will travel the highest

the lightest ion

ane

single

ene

double

yne

triple

saturated

single bonds- easier to break apart

unsaturated

double/triple bonds and have stronger connections making them harder to break apart

is unsaturated or saturated better to eat

unsaturated