exam 3 Flashcards by Max Colby

ionization energy….

increases as the column increases and decreases as you go down a group

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after a full shell, after a half shell

ionization energy drops

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the 5th electron taken out creates a huge jump in energy, what group is this element in?

group 14, (C, Si, Ge,….)

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Electron affinity

energy change from stealing an electron
(ex flourine EA= -349) only negative for the first electron stolen

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electron affinity trend

to the right and up (same full shell half shell trend)

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electrostatic potential energy equation

Eel is proportional to (Q1 x Q2)/d
Q= attraction d = distance

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delocalized

an electron able to travel 3 or more atoms over from the one it came from

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covalent bonds

both elements share electrons evenly due to high ionization energy

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lewis symbol

basically lewis struct but just one element

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cations = anions = (type of energy)

ionization energy. Electron affinity

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larger charges = larger _______

lattice energies

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larger distance = ______ lattice energy

smaller

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Born-Haber cycle

graph to figure out the lattice energy
think deltaH = deltaH1 +deltaH2 +or -…… -lattice energy. in KJ/Mol

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Born-Haber cycle rules

must get to a form that is 1 mole to 1 mol in gaseous state

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lattice energy equation

( Q1 x Q2 ) / distance

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octet rule exemptions

B, P, S, Se, Br, Te, I

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lewis structure rules (6)

count the number of valence
adjust for electron charge
Draw skeleton (central atom with single bonds) (central atom is most electro-positive (Fr is king) and or first)
distribute leftover electrons to other atoms to fill out octet (most electronegative first)
place any remaining on the central atom
if center doesn’t have octet, make double bonds

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check for lewis structure

Complete octets?
formal charges match?
3.multiple lewis structures?
valence structures?

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ionic, polar, nonpolar charge difference

> 1.9, POLAR, <0.4 in electronegativity

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dipole moment

Q (charge) x r (distance). greater difference = greater dipole

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dipole unit

Debyes (D) or (wierd u)

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1 debye =

3.33564 x 10^−30 C·m

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Angstroms

unit of length, 10^-10 meters

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electron charge

1.60 x 10^-19 C

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formal charge

extra electrons that added to the normal valence

formal charges for H2O

H= 0 O=0

charge of _ is perfect, _ is preferable, _ is not correct

0,1,2

if to fill a middle octect with 8 fluorine must become positive _______

this CANNOT happen

when you have multiple lewis structure with same charges possible, choose _______

the more EN element

hypervalence

when in period 3 or lower, to reduce formal charge mid atom can expand the valence

resonance structures

LOOK FOR OXYGENS, equavalent lewis structures that describe a molecule, give ya decimal bond orders

bond order

resonance bonds over amount of bonds (double and single are still one) Plus 1

how to fill out octets

start at the outer and then go inner

Take a moment to memorize vseper models and draw them

oky doky

BOISTERIOUS Boron rules

boron can only have 6 electrons to complete the octet

radical

unpaired electron

S and F compounds

SF2, SF4, SF6

Xe and F compounds

XeF4

higher bond order = ______ angstrums

smaller angstrums, the atoms are closer together

bond enthalpy units and sign

KJ/mol, + (its the energy needed to break the bond)

2 bonds, 0 lone pairs, angle?

linear, 180

3 bonds, 0 lone pairs, angle?

Trigonal Planar, 120

4 bonds, 0 lone pairs, angle?

Tetrahedral, 109.5

5 bonds, 0 lone pairs, angle?

trigonal bipyramidal, 120 and 90

6 bonds, 0 lone pairs, angle?

Octahedral, 90

electron domains

bonds or lone pairs in a compound. (double bonds count as one)

2 bonds, 1 lone pair, angle?

bent or angular, <120

3 bonds, 1 lone pair, angle?

trigonal pyramidal, <109.5

2 bonds, 2 lone pairs, angle?

bent (2) or angular, <<109.5

Vsepr acronym

Valence Shell Electron Pairs Repulsion

4 bonds, 1 lone pair, angle?

Seesaw, <120 and <90

3 bonds, 2 lone pairs, angle?

T-shape, <90

2 bonds, 3 lone pairs, angle?

linear, 180

5 bonds, 1 lone pair, angle?

square pyramid, <90

4 bonds, 2 lone pairs, angle?

square planar, 90

3 bonds, 3 lone pairs, angle?

T-shape, <90

2 bonds 4 lone pairs, angle?

linear, 180

practice drawing vsepr models

oky doky

trigonal bipyramidal where 120 and 90?

the equatorial (three atom ring) = 120, axis position (like the poles of a planet) = 90

which take up more space? lone pair or bond

lone pair

(fill in chapter 9 part that you missed)

oki

sigma bond

first bond, on axis bond, head to head overlap,

Pi bond

off axis bond, side to side overlap, like two faces melting together.

Pi bonds live in ____

P orbitals

sigma bonds live in ____

hybridized orbitals

double bond = ___

Pi bond

single bond = _____

sigma bond

triple bond = ____

sigma AND pi bond

Pi bonds prevents _____

ROTATION of a single side of a molecule

bonding orbital

the orbital that goes to a lower energy level and is constructively interferring (-energy)

antibonding orbital

the orbital goes up and destructively interferes with the bond (+ energy denoted with star *)

node

area where you'll never find an electron. only antibonding orbital has node

bond order calculation

1/2 bonding electrons - antibonding electrons = bond order

hybridization

blending S and P orbitalts

study MOS PI bond structures

oki

diamagnetic (die)

spins of electrons being paired that kill magnetism

paramagnetic

has unpaired electrons that can be lined up to become magnetic

born haber process

the steps to find the lattice energy

a planar molecule

has all of its atoms in the same plane (can ya twist the fucker)

0 unpaired electrons = >0 unparied electrons =

diamagnetic paramagnetic

Angstrom = ?

1x 10^-10 m

delocalized pi bonds have 2 e- per ______ while localized just have _____

p orbital, 2

electron domain vs molecular domain

electron does NOT care about nonbonding pairs. molecular DOES care

exam 3 Flashcards

(84 cards)