Unit 2: Molecular and Ionic Structure and Properties

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108 Terms

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intramolecular forces

attractions within a molecule

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intermolecular forces

attractions between molecules

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ionic bonding

transfer of electrons from a metal to a nonmetal

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coulomb’s law

an increase in charge or decrease in size = increased bond energy

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covalent bonding

sharing of electrons between non metals

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polar molecule

electrons are not shared equally; large change in electronegativity

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nonpolar molecule

electrons shared equally; small change in electronegativity

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repulsion; the molecules are too close to form a bond

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where the molecules are actually bonded together (internuclear distance at this point = bond length)

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where the molecules are too far apart to form a bond

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bond energy

bond energy

<p>bond energy</p>
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strongest bond

lowest potential energy = ?

<p>lowest potential energy = ?</p>
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smaller

bond length is shorter for _______ molecules

<p>bond length is shorter for _______ molecules</p>
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increased bond energy, decreased bond length

increased bond order = ?

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bond order

the number of bonding pairs of electrons between two atoms

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from sp to sp³

<p></p>
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sp³

what is the hybridization of oxygen?

<p>what is the hybridization of oxygen?</p>
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pi bonds

formed by the lateral overlap of two atomic orbitals; e-shared around atoms

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sigma bonds

a result of the head-to-head overlapping of atomic orbitals; e- shared between atoms

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8 sigma, 3 pi

sigma bonds and pi bonds?

<p>sigma bonds and pi bonds?</p>
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2 sp³ orbitals

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yes, from sp to sp²

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bond polarity

difference in electronegativity of two elements

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more electronegative atom

dipole arrow points towards ______

<p>dipole arrow points towards ______</p>
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increased bond energy

delocalized electrons = ____________

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single bond

sigma bond

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double bond

sigma bond + pi bond

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triple bond

sigma bond + 2 pi bonds

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Octet rule

All atoms end up with 8 electrons around them (except for hydrogen and boron)

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Steps to draw Lewis Structures

  1. count the valence electrons of all the atoms

  2. determine the central atom

  3. remove an electron from each atom for a bond (S—O bond removes one electron from S and one from O)

  4. add the remaining electrons as lone pairs to create an octet around each atom

    1. if octet has not been achieved add multiple bonds

    2. if all atoms have achieved an octet and not all valence electrons have been assigned, add the remaining electrons to the central atom

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most electronegative

the central atom is the ______

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expanded octet

when a atom has more than 8 electrons

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the electrons of pi bonds are delocalized

in resonance structures

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formal charge

a hypothetical charge assigned to an atom in a molecule. It's based on the assumption that electrons in all chemical bonds are shared equally between atoms, regardless of their relative electronegativity.

= valence electrons - (lone electrons + ½ bond electrons)

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better structures

molecules with lower formal charges are _____

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negative

a more electronegative atom will have a more _______ formal charge

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sign

adjacent atoms should not have formal charges with the same ________

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charge on chemical species

sum of formal charges =

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closer to 0

a more favorable Lewis Structure will have a formal charge ___________

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0

6 valence electrons - (4 unbonded electrons + 4 bond electrons / 2) = 0

formal charge of oxygen in H2O

<p>formal charge of oxygen in H2O</p>
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0

6 valence electrons - (4 unbonded electrons + 4 bond electrons/2) = 0

formal charge of oxygen in CO2

<p>formal charge of oxygen in CO2</p>
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0

4 valence electrons - (0 unbonded electrons + 8 bond electrons/2) = 0

formal charge of carbon in CO2

<p>formal charge of carbon in CO2</p>
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0

1 valence electron - (0 unbonded electrons + 1 bond electron/2) = 0

formal charge of hydrogen in H2O

<p>formal charge of hydrogen in H2O</p>
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-1

6 valence electrons - (6 unbonded electrons + 2 bond electrons/2) = -1

formal charge of oxygen furthest to the left in NO3

<p>formal charge of oxygen furthest to the left in NO3</p>
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-1

charge of resonance structure

<p>charge of resonance structure</p>
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the one on the left, because it has a charge of 0

which resonance structure is more favorable?

<p>which resonance structure is more favorable?</p>
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negative

bonds and lone pairs are ________

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repel

electrons (-) ____ each other

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minimize repulsion

because bonds and lone pairs are negative, they arrange themselves to ________________

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steric number

number of electron domains

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2

sp steric number

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3

sp² steric number

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4

sp³ steric number

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Linear

<p></p>
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180
Linear bond angle
Linear bond angle
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2
Linear (# of electron domains)
Linear (# of electron domains)
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Linear
Linear Basic Geometry
Linear Basic Geometry
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trigonal planar
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120
trigonal planar bond angle
trigonal planar bond angle
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3
trigonal planar # of electron domains
trigonal planar # of electron domains
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trigonal planar
Trigonal planar basic geometry
Trigonal planar basic geometry
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bent
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< 120
bent bond angle
bent bond angle
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3
bent (# of electron domains)
bent (# of electron domains)
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trigonal planar
bent basic geometry
bent basic geometry
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Tetrahedral
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109
tetrahedral bond angle
tetrahedral bond angle
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4
Tetrahedral (# of electron domains)
Tetrahedral (# of electron domains)
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tetrahedral
tetrahedral basic geometry
tetrahedral basic geometry
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trigonal pyramidal
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trigonal pyramidal bond angle
trigonal pyramidal bond angle
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4
trigonal pyramidal (# of electron domains)
trigonal pyramidal (# of electron domains)
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tetrahedral
trigonal pyramidal basic geometry
trigonal pyramidal basic geometry
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bent (tetrahedral)
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<< 109
bent (tetrahedral) bond angle
bent (tetrahedral) bond angle
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4
bent (tetrahedral) (# of electron domains)
bent (tetrahedral) (# of electron domains)
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tetrahedral
bent (tetrahedral) basic geometry
bent (tetrahedral) basic geometry
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trigonal bipyramidal
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120, 90
trigonal bipyramidal bond angle
trigonal bipyramidal bond angle
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Sawhorse or Seesaw (trigonal bipyramidal)
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< 90, < 120

Sawhorse or Seesaw (trigonal bipyramidal) bond angle

<p>Sawhorse or Seesaw (trigonal bipyramidal) bond angle</p>
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T-shape (trigonal bipyramidal)
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< 90
t-shape (trigonal bipyramidal) bond angle
t-shape (trigonal bipyramidal) bond angle
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linear (trigonal bipyramidal)
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180
linear (trigonal bipyramidal) bond angle
linear (trigonal bipyramidal) bond angle
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octahedral
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90
octahedral bond angle
octahedral bond angle
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square pyramidal
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< 90, < 90

square pyramidal bond angle

<p>square pyramidal bond angle</p>
90
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square planar
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90
square planar bond angle
square planar bond angle
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T-shape (octahedral)
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< 90

T shape (octahedral) bond angle

<p>T shape (octahedral) bond angle</p>
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linear (octahedral)
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180

linear octahedral bond angle

<p>linear octahedral bond angle</p>
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polar molecule

a molecule with an uneven distribution of charges; asymmetrical; bonds don’t cancel out; lone pairs of electrons disrupt electrical symmetry

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nonpolar molecule

a compound with an even distribution of charges; symmetrical; identical atoms

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polar; the lone pairs on the oxygen atom make the molecule asymmetrical

polar or nonpolar?

<p>polar or nonpolar?</p>
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nonpolar, because it has an even distribution of electron density, and its dipoles cancel each other out. 

polar or nonpolar?

<p>polar or nonpolar?</p>
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polar

any molecule with lone pairs of electrons on the central atom