CHEM 1211K: Unit 4 Quiz

v

v

1/5=hz

frequency

λ

wavelength; nanometer, angstrum

c

speed of light; 3*10^8 meters/second

d

orbital; clover leaf or maybe a dumbbell with a donut around it

f

orbital; bigger

h

converts frequency of light to energy of light; planks constant

l

type of orbital; 0-n-l; l=0=s; which type of orbital you’re in (s,p)

Resonance Structures

two different lewis structures but are equivalent; ability to have two lewis structures correct enough to matter;

m sub l

-l or +l

n

shell, quantum numbers; borrs only 1, counting numbers

p

orbital

s

orbital, sphere, only 1

m sub s

spin= +1/2 or -1/2

E=hv

photon; planks constant

c=vλ

speed of light, frequency and wavelength

relationship between speed, frequency and wavelength of light

sigma

+ ee + ; squishes orbitals to create new orbitals

pi

e e

+ +

___

a bond which exists above and below space of atom

anti-bonding

cancels out full on bond; electrons on wrong side of nucleus; pulls apart; sigma and pi

electronegativity

bottom left to top right; francium to fluorine; how attracted electrons are to each other. bottom is least electronegative fluorine is most electronegative

first ionization energy

energy required to remove loosely held electron; fluorine

spin

m sub s is quantum number for spin

hybrid orbital

only looks at valence electrons; way of simplifying orbitals

ground state

packed electrons into lower orbital

excited state

every enters electron and kicks electron to higher state; doesn’t last long; may have a better set of quantum numbers

bond association enthalpy

energy it takes to pull 2 bonds apart

bent

a kind of molecular geometry in which the central atom has two lone pairs of electrons and is associated with two bond pairs; also known as angular or V-shaped; between 104-109.5º

photon

particle of light

polar

fairly decent difference between electronegativity between a bond

nonpolar

a molecule with polar bonds that is symmetrical

shell

home for electrons; found around nucleus

orbital

a wave function

describes properties characteristic of no more than two electrons in the vicinity of an atomic nucleus or of a system of nuclei as in a molecule

s,p,d,f

lone pair

a pair of valence electrons that are not shared with another atom

linear

has an angle of 180º; molecules that are straight; ex: CO2; BeH2

trigonal planar

a central atom connected to three atoms arranged in a triangular pattern around the central atom; 120º; Ex: SO3

tetrahedral

109.5º; four bonds and no lone pairs in the molecule's central atom; ex: CH4

trigonal pyramidal

three bonds and one lone pair on the central atom in the molecule; <109.5º, ex: NH3

trigonal bipyrimidal

five bonds and no lone pairs on the central atom in the molecule; 90º or 120º, ex: PCl5

seesaw

central atom has one lone pair of electrons and is coupled to four bonding groups; 90º-120º; ex: SF4

t-shaped

central atom has three ligands; 90º; ex: ClF3

octahedral

six atoms or groups of atoms or ligands symmetrically arranged around a central atom, defining the vertices of an octahedron; 90º; ex: Mo(CO)6

square planar

lone pairs of electrons on opposite sides of the central atom; 90º; ex: XeF4

square pyramidal

five bonds and one lone pair on the central atom in the molecule; 90º; ex: BrF5

atomic size

the distance between the centre of the nucleus of an atom and its outermost shell

molecular orbital

mathematical function describing the location and wave-like behavior of an electron in a molecule

quantum number

describe values of conserved quantities in the dynamics of a quantum system; ex: n, l

wave

shape that alternatively varies between a maximum in two opposite directions; ROYGBIV

particle

the microscopic constituents of matter like nuclei of atoms

valence

the property of an element that determines the number of other atoms with which an atom of the element can combine; last shell of electron is valence shell

core

electrons in an atom that are not valence electrons and do not participate in chemical bonding

isomer

compounds that have the same molecular formula but are structurally different

120º

trigonal planar

180º

linear

109.5º

tetrahedral