Exam 3: Definitions Flashcards

1
Q

Ionic compounds

A

Metal + nonmetal

dissolves in water

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2
Q

molecular compound

A

nonmetals

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3
Q

Electronegativity

A
    | ----> 

right and up. Top right

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4
Q

increasing boiling point

A

more bonds = more energy to melt

H bonds are weak but H-H bonds are weaker

double/tripple bonds = more energy to break

bigger size = more energy to break

more heat = more breaking of bonds

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5
Q

The numerical value of an element’s electronegativity represents….

A

the ability of an atom in a bond to draw shared electrons to itself

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6
Q

Radical

A

1 atom has an odd number of electrons (after bonding everything after)

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7
Q

dipole- dipole

A

Next strongest

attractive forces between the positive end of one polar molecule and the negative end of another polar molecule

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8
Q

Hydrogen bonding

A

Can attract other molecules that are SIMILAR

ONLY occurs between molecules with Hydrogen bonded to high electronegative elements like N, O, F

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9
Q

london dispersion forces

A

Weakest bond compared to dipole-dipole and hydrogen bonding

everything is attracted to the dispersion force (bigger molecule = bigger dispersion force)

weak = gas
strong = solids

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10
Q

Electron domains

A

lone pairs,
single, double, tripple bonds

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11
Q

valance bond theory describes how a covalent bond is formed by….

A

the overlap of two orbitals, with each orbital containing one electron

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12
Q

polar

A

dipole

London dispersion and dipole-dipole

lower it is on PT = lower polarity

Polar/ Polar covalent (e shared UNequally) : .5-2

BOTH need to be met or else its non-polar:

1)central atom has no lone pairs

2)all atoms around the central atom are the same

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13
Q

non-polar

A

no dipole

London dispersion

ONLY ONE needs to be met:

1) the central atom has no lone pairs

2) all atoms around the central atom are the same

Non-polar / covalent (e shared equally): less than .5

has symmetry

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14
Q

dipole

A

based on electronegativity
difference in electrons

lightly charged on one side than other

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15
Q

When a covalent bond forms between two atom, the potential energy of the system ______. To break a bond, energy must be ______.

A

Decrease
added

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16
Q

Octet rule states

A

atom gains, lose, or share electrons so that they end up with a full outer shell

17
Q

valence bond theory describes how a covalent bond is formed by…

A

the overlap of two orbitals, with each orbital containing one electron

18
Q

lone pairs

A

2 electrons (pair)

19
Q

Polyatomic ions

A

Charged ions

20
Q

Resonance

A

when two or more L.S with atoms in the same position are averaged to gove the true structure

21
Q

The ability of a bonded atom to draw shared electrons to itself is called…

A

electronegativity

22
Q

Boiling point question: atmosphere pressure and room temp, bromine is a liquid, and iodine is a solid. we can conclude that bromine….

A

has weaker intermolecular forces that iodine

(bromine is weaker cuz bonds broke and turned into liquid)

23
Q

Attractions

A

Like attractions: repel
Opp attractions: attract

24
Q

When a covalent bond forms between two atoms, the potential energy of the system ______. to break a bond, energy must be _____.

A

decreases
added

25
Q

Periodic table movements

A

+ means move left

  • means move right
26
Q
A
27
Q

Lewis Structure movements

A

Add electrons for NEG charges

Sub electrons for POS charges

28
Q

Lewis structure drawing additions

A

+ for Lewis structure if L.S needs to LOSE electrons

– for Lewis structure if L.S needs to GAIN electrons

29
Q

ion-induced dipole

A

attraction between ionic and nonpolar

30
Q

Ion-dipole

A

Atrraction between ionic and polar

31
Q

Covalent bonds

A

SHARED bonds, not transfer

32
Q

intermolecular forces

A

keeps everything tohether

33
Q

polymers

A

chain of repeating molecules

34
Q

Distinguish if bonds are polar, non-polar, or ionic

A

Polar/ Polar covalent (e shared equally) : .5-2
Non-polar / covalent (e shared UNewually): less than .5
Ionic (transferred bonds) : 2.0 or more

35
Q

Compounds with H-F, H-N

A

London dispersion, dipole-dipole, hydrogen bond