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Chemistry 111 > chem test 2 > Flashcards

chem test 2 Flashcards

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1
Q

covalent bond

A

pair of shared electrons

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2
Q

polar covalent bond

A

pair of shared electrons with the electron pair lying closer to 1 atom than to the other atom

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3
Q

electronegativity (Linus Pauling)

A

measure of how strongly atoms pull electrons
on periodic table, electronegativity increases to the right and up
Χ (chi) is the symbol

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4
Q

dipole moment

A

mu, is measure of HOW polar a polar bond is

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5
Q

resonance

A

when there is more than 1 way to arrange the double and/or triple bonds in the lewis structure. the actual structure is an average (hybrid) of different resonance structures

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6
Q

free radical

A

molecule or ion which has 1 or more unpaired electrons

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7
Q

formal charge (fc)

A

group# - # of bonds - # nonbonding electrons

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8
Q

electroneutrality principle (Linus Pauling)

A

if there is resonance, the preferred structure is the one with the smallest set of formal charges, and the one that has the most negative formal charges on the most electronegative atom

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9
Q

which bond is strongest

A

triple bond

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10
Q

which bond is longest

A

single bond

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11
Q

**VSPER

A

valence shell electron pair repulsion theory

electron pairs have negative charge, and try to spread themselves out as far as possible

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12
Q

equatorial positions

A

those in the main plane of molecules

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13
Q

axial positions

A

those above and below the main plane of molecules

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14
Q

polar bond

A

bond between atoms with different electronegativities

1 side of the bond is different from the other side of the bond

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15
Q

electron group

A

“things attached”

an electron, pair of electrons, 1 bond, multiple bonds

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16
Q

bonding group

A

a bond, single double or triple

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17
Q

lone pair

A

pair of electrons not involved in bonding

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18
Q

valence bond

A

pair of shared electrons produced by overlapping atomic orbitals from 2 different atoms

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19
Q

solution to bond angle issue for valence bonds

A

hybrid orbitals-linus pauling

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20
Q

sigma bond

A

pair of shared electrons mainly in the axis between the 2 atoms

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21
Q

pi bond

A

has the pair of shared electrons mainly above and below the bond axis

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22
Q

molecular orbitals

A

orbitals which extend over the whole molecule (or at least 1 bond) rather than just an atom
orbitals tell us where electron is likely to be

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23
Q

four principles of molecular orbital theory

A

of molecular orbitals=# of bonding atomic orbitals
bonding MO is always a lower energy than the antibonding MO
electrons are assigned to MOs using the Pauli principle and Hunds rule
usually, MOs are made from atomic orbitals of approximately the same energy

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24
Q

*molecular orbital antibonding because

A

the main electron density is outside the atom, pulling them apart

25
Q

how many electrons in an orbital

A

2, one with spin up and one with spin down

26
Q

diamagnetic

A

all electrons spin paired

27
Q

paramagnetic

A

one or more electrons is NOT spin paired

28
Q

bond order for molecular electron configuration

A

(electrons bonding MO - electrons antibonding MO) / 2

29
Q

replacement reactions

A

HOH->NaOH

30
Q

delta symbol

A

means heat supplied

31
Q

decomposition reaction

A

(NH4)2Cr2O7(s)->NH3+CrO3+H2O (not balanced)

32
Q

(aq)

A

aqueous/soluable

33
Q

replacement reaction

A

Cu+AgNO3->Ag+Cu(NO3)2

34
Q

up arrow

A

gas formed

35
Q

double replacement reaction

A

AB+CD->AD+CB

36
Q

stoichiometry

A

weight-weight relationships

37
Q

limiting reagent (reactant)

A

the reactant that is all used up in a reaction, and determines when the reaction is stopped

38
Q

percent yeild

A

actual/theoretical x 100

39
Q

solution

A

homogenous mixture of 2 or more components

40
Q

solvent

A

major component of the solution

41
Q

solute

A

minor component

42
Q

aqueous solution

A

the solvent is water

43
Q

molarity

A

the way concentrations are measured, moles of solute per liters of solution
M=n/V

44
Q

strong electrolyte

A

conducts electricity well

45
Q

what kinds of solutes produce weak/strong electrolyte solutions

A

all salts are strong electrolytes (1 positive and 1 negative)
strong acids are strong electrolytes, all other acids are weak (acetic)
strong bases are strong electrolytes, all other bases are weak

46
Q

strong acids

A

HNO3, H2SO4, HCl, HBr, HI, HClO4

47
Q

strong bases

A

alkaline metal hydroxides, NaOH, KOH, LiOH, Ca(OH)2, Sr(OH)2 Ba(OH)2, Mg(OH)2

48
Q

solubility rules

A

Na+, K+, NH4+, are soluble
NO3-, F-, C2H3O2- are soluble
SO4-2 are soluble EXCEPT Ba2+, Sr2+, Ca2+, Pb2+, Ag2+
Cl-, Br-, I- are soluble EXCEPT Ag+, Pb2+, Hg22+
everything else is insolube

49
Q

metathesis reaction

A

double replacement, with at least one of the products insoluble, gas, or water

50
Q

spectator ion

A

ion that appears on both sides of ionic equation

51
Q

acid

A

anything that provides H+(aq) ions in solution

52
Q

strong acid

A

strong electrolyte, conducts electricity, dissociated ions

53
Q

polyprotic acid

A

multiple H

54
Q

diprotic acid

A

2 H

55
Q

base

A

substance that provides OH-(aq) ions in solution

56
Q

acid base titration

A

acid is slowly added to base, or vice versa, until all has been neutralized. the molarity of the H+ must be equal to the molarity of the OH-

57
Q

oxidation reaction

A

originally, reaction of anything with oxygen

currently, oxidation is a reaction in which the oxidation # of something increases

58
Q

oxidation-reduction reaction

A

reaction in which the oxidation # of 1 element increases and the oxidation number of another element decreases

59
Q

rules for determining oxidation numbers

A
  1. oxidation # of any element by itself is 0
  2. the oxidation # of a monatomic ion is it’s charge
  3. hydrogen has an oxidation # of +1, oxyden has a # of -2
  4. sum of the oxidation numbers in a molecule add up to 0
  5. sum of the oxidation numbers in an ion is it’s charge

Chemistry 111 (7 decks)

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