chapters 3 and 4 Flashcards by Ally Carpenter

ionic bonding

the complete transfer of valence electrons

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covalent bonding

sharing of electrons

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polar bonds

unequal sharing of electrons

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general trend of electronegativity

increases going left to right and up a column

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VSEPR theory

structures surrounding and atom is determined by minimizing electron pair repulsions

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chemical bond

force that holds atoms together

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bond energy

required energy to break a bond

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bond length

distance where energy is minimal

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nonmetallic elements achieve a noble gas configuration by _____ electrons

sharing

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metals are _____

cations

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nonmetals are _____

anions

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cation is generally _____ than parent atom

smaller

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anions are generally _____ than parent atom

larger

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ion size______ going down a group

increases

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ions generally adapt ______ configurations in ionic compounds

noble gas electron

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isoelectronic ions

ions containing the same number of electrons

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______ protons means ______ attraction and _______ ions

more, greater, smaller

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electronegativity

ability of an electron to attract shared electrons to itself

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lattice energy

change in energy that takes place when separated gaseous ions are packed together to form an ionic solid

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all compounds with _____% or more ionic character are considered to be ionic solids

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delocalization of electrons

eletrons free to move through entire molecule

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as number of shared electrons _____ bond length _____

increases, shortens

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energy terms with bond breaking have a ____ sign

positive

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energy terms with bond making have a ___ sign

negative

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list the exceptions to the octet rule

boron, and any row 3 or lower

resonance

when more than one correct lewis structure can be drawn

formal charge formula

valence-non bonding-bonding/2

valence electron formula

lone pairs+ 1/2(shared electrons)

how to name type 1 compounds

cation first anion 2nd cation takes name from element anion named by taking root of element name and adding -ide

how to name type 2 compounds

same as type one cation first then anion must specify the charge add -ide to the end

how to name type 3 compounds

first element named with full name 2nd element named like anion prefixes for the nunber of atoms mono prefix not used for first element

molecular structure

3d arrangement of atoms in a molecule

2 pairs of electrons means what shape

linear

3 pairs of electrons means what shape

trigonal planar

4 pairs of electrons means what shape

tetrahedral

5 pairs of electrons means what shape

trigonal bipyramidal

6 pairs of electrons means what shape

octahedral

true or false in vsper a double bond is counted as one effective pair

true

dipole moment

molecule with a center of positive and negative charge

electrostatic potential diagram

colors of visible light are used to show the variation in charge distribution red= electron rich blue= electron poor

hybridization

mixing of native atomic orbitals to form special orbitals for bonding

sigma bond

electron pair is shared in an area centered on a line running in between the atoms

pi bond

parallel p orbitals that occupy space above and belowine joining atoms

in a single bond how many sigma bonds are there

in a double bond there is ____ sigma and ____pi

1 and 1

in a triple bond there is ____ sigma and ___pi

1 and 2

bond order

(bonding electons-antibonding electrons)/2

_____ bond order means ____bond strength

larger, greater

paramagnetic

unpaired electrons make something paramagnetic

diamagnetic

when all electrons are paired

as bond order _____ bond energy _____ and bond length _____

increases, increases, decreases

is o2 paramagnetic or diamagnetic

paramagnetic

electron geometry

includes lone pairs and bonding electrons

molecular geometry

includes only bonding pairs

nonpolar

if molecule has a symmetric shape and like bonds

formal for change in E

change in E=bonds broken-bonds formed

ionic bonds generally form between what

metals and nonmetals

to choose best lewis structure using formal charge the charge of the central atoms should be close to ____

zero

what shape has sp hybridization

linear

what shapes have sp2 hybridization

bent and trigonal planar

what shapes have sp3 hybridization

tetrahedral, seesaw, trigonal pyramidal

what shapes have sp3d hybridization

trigonal bipyramidal

what shape has sp3d2 hybridization

octahedral

ammonium

NH4+

carbonate

CO3^2-

chlorate

ClO3-

chromate

CrO4^2-

cyanide

CN-

hydroxide

OH-

nitrate

NO3-

phosphate

PO4^3-

sulfate

SO4^2-

permanganate

MnO4-

type 2 compounds typically involve....

transition metals

type 3 compounds are made of...

two nonmetals

type 1 compounds always have...

a cation and anion

single bond has a bond order of

double bond has a bond order of 2

triple bond has a bond order of 3