unit 2 test Flashcards by Kia Thomas

how do you determine central atom

least electrognegative

listed 1st in formula

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when making lewis diagrams

add up all the VE for the compound
add up ionic charges also

(negative charge means add electrons and positive charge means take away electrons)

for ions also put square brackets and the charge on the outside

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a line between dots represents

a shared pair of electrons forming. a single covalent bond

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ionic bonds are stronger when

charges are larger and ions are smaller

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metallic bonding

occurs between metal bonds

metal attractions due to cations being attracted to a de localized sea of electrons

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alloys

mixtures of metals

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interstitial alloys

atoms added to metals are small and fit between metal atoms, in hole(interstices)

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substitutional alloys

atoms added to metal have similar radii so they replace atoms in lattice

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which atoms have expanded octets

and what are octets

central atom has more than 8 around it

3rd periods and below have expanded octet

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bond length influenced by

the size of atoms core and bond order

bonds w a higher order are shorter and have larger a bond energies

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interaction strength is proportional to

charge of each ion

large charges leas to stronger interactions

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covalent bonds occur at

lowest energy state

attractions between nuclei is greatest for shared electrons

repulsión a between electrons and between the nuclei is the least

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isomer

same number and type of atoms but different arrangements

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large atomic radii increases..

bond length

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long bond length decreases…

bond energy

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for electrons to be conduct electricity they need to be

free moving/flowing

particles need to be charged

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what does VSEPR stand for

valence shell electron pair repulsion

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how do lone pairs affect the bond angle

increase the repulsion

bring other atoms closer together so the bond angle is smaller

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what does hybridization and hybrid atomic molecule describe?

arrangement of electrons around a central atom

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electron domains

single bond, double bond lone pair, etc all count for an individual electron domain

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sp2

how many s and p orbitals

how many electron domains

1 s orbital, 2 p orbitals

3 electron dominas

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Electrons involved in binding among metal atoms are

Equally shared and NONdirectional bonds

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For the potentials energy graphs

Would cl be outside or inside the graph of br

Cl is higher up(vertically),above br

Outside graph of br

Smaller atomic radius means more outside, greater graph

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For the potentials energy graphs

Would F be outside or inside the graph of C
F is more to the right, than C horizontally on the periodic table

Outside the graph of C

Smaller atomic radius means more outside, greater graph

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What is the hybridization of 3 areas w/ electrons or a double bond

Sp^2

2 areas w/ electrons or triple bonds

4 electron areas (single bond)

Sp^3

What is bond order

Bond order is the # of bonding pairs of e- between 2 atoms A single bond has a bond order of of 1

what do metal elements have with their e-

a sea if electrons

electronegativity of pure covalent

less than .4

electronegatovity of polar covalent bonds

0.4-1.8

ionic bonds eñectrongetivity

greater than 1.8

polarity

difference greater than .5

ionic bonds, electrons are

transferred from cation to anion

what are ionic solids called

salts

covalent bonds electrons are

shared between atoms

which direction does the dipole arrow point

towards the more electronegative atom

unstable bond | would look at graph

potential energy greater than 0

stable bond | would look at graph

potential energy less than 0

y-axis of graphs

energy required to break the bond(endothermic process)

x-axis of graph

distance between atoms, bond length

use peale of graph to determine

bond energy and length

greater lattice energy

consider ionic radius- smaller IONIC radius means higher lattice energy because ions can get closer together consider distance between elements horizontally (greater charge difference means greater lattice energy)

octet rule

except for H and B all atoms should end up with 8 electrons around them

how to determine center atom of molecule

the first written ir the most electronegative(upper right corner)

HONC | 1234

means at most those atoms can have that many electrons(they can have less) usually carbon does have 4 however

best or most dominant lewis diagrams

have a total formal charge of 0 or most negative formal charge should go to the most electronegative element

how to find formal charge

#of total VE minus individual VE in that diagram minus # of bond in that diagram

what does VSEPR

valence shell electron pair repulsion

each electron domain counts equally no matter the...

bond order(single, double, etc.(

what do lone pairs do to an electron structure

they take up more space, changing the shape of the bond because the other electrons are repelled by the lone pairs causing the other electrons to be closer together

nonpolar molecules

lewis diagram is symmetrical

polar molecules

lewis diagrams have lone pairs

how to find hybridization

electron domains minus one

double bond hybridization

sp2 3 electron domains usually ; 3 areas with electrons USUALLY

triple bond

sp2 2 areas with electrons usually

4 electron areas

sp3

if there is a C-C bond in the center or more (C-C-C, C-C-C-C,..) then..

count it as a single central atom pretend or redraw the element as a central atom to find the appropriate hybridization

Lattice energy

Liek bond energy | Energy required to completely separate one mole of solid ionic compounds into gaseous ions

Ionic substance What are there boiling points

High melting and boiling points

Do ionic solids conduct electricity

No they do not conduct electricity

How do ionic compounds act in polar solvents or non polar solvents Solubility?

Soluble in polar solvents Insoluble in non polar solvents

Elements in 3rd period can do what with their octet

Expand their octet, have more than 8 electrons when they are the central atom

The bond length in resonance is

The average of the bonds present

Sigma bond is formed from

Overlapping orbitals from a single bond

Pi bonds are formed from

Unhybridized p orbitals with double and triple bonds

Equation for resonance drawing

#of bonds/# of atoms it’s shared by 3/2 A double bond and a single bond between Oxygen

single sigma bond

double sigma bond

triple sigma bond

single pi bond

double pi bond

triple pi bond

zero dipole moment

no partial charge on either end of the covalent bond

does SO2 have a dipole moment

no because they both have the same charge (-2)

NF3 hybridization

sp^3 lone park counts as electron domain also electrons domains(4) - 1 = 3

valence electrons shared between atoms of similar electoronegativoty constitute a

non polar covalent bond

when considering whether a structure is polar HCN

consider if the shape is symmetrical then also consider electronegativity , dipole moments polar

when reading potential energy vs inter nuclear distance graphs consider

the first part where the graph crosses the x axis and that aligns with bond length (not the last part)

stable point of potential energy graph

lowest point of potential energy graph

unit 2 test Flashcards

(80 cards)