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chem test Flashcards

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1
Q

2 bonded atoms, 0 lone pairs

A

linear, 180, 2 total electron domains

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2
Q

domain

A

a location of a bond or a lone pair of electrons (double and triple bonds only count as one domain)

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3
Q

3 bonded atoms, 0 lone pairs (Boron triflouride; BF v 3)

A

trigonal planar, 120, 3 total electron domains

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4
Q

2 bonded atoms, 1 lone pair (Nitrate Ion; NO v 2 ^ -1)

A

bent, 118, 3 total electron domains

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5
Q

4 bonded atoms, 0 lone pairs (Methane; CH v 4)

A

tetrahedral, 109.5, 4 total electron domains

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6
Q

3 bonded atoms, 1 lone pair (Ammonia; NH v 2)

A

trigonal pyramidal, 107, 4 total electron domains

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7
Q

2 bonded atoms, 2 lone pairs (water; H v 2 O)

A

bent, 104.5, 4 total electron domains

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8
Q

5 bonded atoms, 0 lone pairs (PCl v 5; Phosphorus pentachloride)

A

trigonal bipyramidal, 120 and 90, 5 total electron domains

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9
Q

6 bonded atoms, 0 lone pairs (Sulfur nexaflouride; SF v 6)

A

octahedral, 90, 6 total electron domains

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10
Q

diatomic ions, and what elements can form them

A

ions made up of two atoms of the same element. They are always found together in a compound. The following elements can form diatomic ions: H, N, O, F, Cl, Br, and I.

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11
Q

monatomic ions

A

are ions formed from a single atom. They can be either positive or negative.

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12
Q

cation

A

ion that has lost electrons and has a positive charge (cat–> PAWsitive)

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13
Q

anion

A

ion that has gained electrons and has a negative charge

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14
Q

ion

A

An ion is an atom or a group of atoms that has gained or lost electrons, resulting in a positive or negative charge

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15
Q

what follows single element cations? for example Na ^ +

A

the name of the element is used followed by the word word “ion”
Na ^ + = sodium ion

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16
Q

what follows single element anions? for example Cl ^ -

A

the name of the element is used followed by the suffix “-ide”
Cl ^ - = chloride ion

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17
Q

how do you write a single element transition metal ion? for example Fe ^ 3+

A

you have to include the charge in roman numerals following the element name
Fe ^ 3+ = iron (III) ion

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18
Q

NH v 4 ^ +

A

ammonium

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19
Q

SO v 3 ^ 2-

A

sulfite

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20
Q

SO v 4 ^ 2-

A

sulfate

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21
Q

OH -

A

hydroxide

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22
Q

PO v 4 ^3 -

A

phosphate

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23
Q

O v 2 ^2 -

A

peroxide

24
Q

how do you write and name ionic bonds? for example Na+Cl-

A

criss cross their charges down (to achieve neutrality)
Subscripts must be the lowest ratio when canceling charges.
positive metal ion always comes first
drop the second syllable of the negative/anion element and subsitute with “-ide”
Na+Cl- = NaCl
sodium + chlorine = sodium chloride

25
Q

ionic compounds must have an overall ______ charge

A

neutral (charge of 0)

26
Q

what are ionic compounds made of?

A
  • Ionic compounds are formed when positive and negative ions combine.
  • have a metal and a nonmetal
27
Q

how do you name transition metal ionic compounds? for example CuO vs Cu v 2 O

A

you include the roman numeral in the name
CuO = copper (I) oxide
Cu v 2 O = copper (II) oxide

28
Q

polyatomic ions

A

most polyatomic ions are covalent
ions that are made with more than two elements (SO v 4 ^ 2- = sulfate)
- when you do the drop and switch (criss cross), use parenthesis
ex: Ca ^ 2+ + NO v 3 ^ -1 = Ca(NO v 3) v 2
use both names –> calcium nitrate
if there are two polyatomic you use both of them as well –> ammonium oxalate

29
Q

ionic compounds with transition metals; for example
Cu ^ +2 Cl ^ -1

A

CuCl v 2 = copper (II) chloride
make sure to specify the charge of the transition metal with roman numerals
(re criss crossing )

30
Q

covalent compounds are made of ______

A

two or more nonmetals SHARE electrons

31
Q

how do you name covalent bonds? for example SO

A

prefixes are used to indicate the number of atoms in each element
- end second element with “-ide”
- mono is NOT used for the first element
- sulfur monoxide

32
Q

prefixes

A

1- mono
2- di
3- tri
4- tetra
5- penta
6- hexa
7- hepta
8- octa
9- nona
10- deca

33
Q

VSEPR

A

valence shell electron pair repulsion
- The model states that electron pairs will repel each other such that the shape of the molecule will adjust so that the valence electron-pairs stay as far apart from each other as possible.
- VSEPR theory allows more accurate predictions of molecular shape

34
Q

intermolecular

A

attractive force between molecules (dipole= polarity)

35
Q

different types of IMF (intermolecular forces)
put them from strongest to weakest

A

hydrogen bonding
dipole-dipole attraction
london dispersion attraction

36
Q

dipole-dipole attraction

A

occurs between : partially oppositely charged ions
relative strength: strong

37
Q

hydrogen bonding

A

occurs between : H atom and O, N or F atom
relative strength: strongest of the dipole- dipole attraction

38
Q

london dispersion attraction

A

occurs between: temporary or induced dipoles
relative strength: weakest

39
Q

metallic bond diagram

A

sea of e- (reason for conductivity)

40
Q

lone pair

A

a pair of valence electrons that are not shared between atoms (aka nonbonding pair or unshared pair )

41
Q

single pair

A

bond between two atoms by one pair of electrons

42
Q

double pair

A

bond between two atoms by two pairs of electrons

43
Q

triple bond

A

bond between two atoms by 3 pairs of electrons

44
Q

what type of bond are
H v 2 O
NaCl

A

H v 2 O = bent because it has one bond
- covalent, polar

NaCl = linear because it only has 2 pairs
- ionic

45
Q

types of covalent bond types

A

polar and nonpolar

46
Q

polar

A

typically between two different elements
- electrons are more on one side than the other (toxic bf)

Sharing of electrons: unequal attraction for electrons so the sharing is UNEQUAL

electronegativity difference: 0.4-1.7
_____>
examples: HF H F

47
Q

non polar

A

Sharing of electrons: shared equally between the two atoms

Electronegativity difference: less than 0.4

examples: Cl Cl—–> Cl v 2

48
Q

octet rule

A

atoms prefer to have 8 electrons in the valence shell

49
Q

lewis dot diagrams

A
  • atomic models which show valence electrons and can be used to predict bonding
  • bonding occurs when atoms try to reach octet
50
Q

ionic compound (characteristics)

A
  • lattice structure of atoms, transfer of electrons

conductivity: electrons are FIXED, no conductivity in solids, conductivity in liquid

solubility: many are soluble in H v 2 o

state of matter: crystaline solids

other: large electronegativity difference between ions (greater than 1.7)

electrons: transferred from metal to non-metal. elements attracted by opposite charges

51
Q

covalent compound (characteristics)

A
  • sharing of electrons

conductivity: no conductivity

solubility: most are non soluble in H2O, soluble in nonpolar solvents

state of matter: liquid or gas at room temperature

other: small or no difference in electronegativity between atoms (less than 1.7: polar 0.4-1.7; non-polar 0-0.4)

electrons: shared between 2 nonmetals

52
Q

Metallic compound (characteristics)

A
  • sea of electrons (e-)

conductivity: good conductivity

solubility: most do not dissolve in H2O, some react with H2O

state of matter: solid at room temperature, mercury at room temp is a liquid

other: most metallic bonds are made of the same atoms so electrons are shared equally
- alloys are mixtures of metals

53
Q

alloys

A

mixtures of metals

54
Q

electronegativity

A

the tendency of an atom to attract electrons to itself in a chemical bond

55
Q

what occurs when salt dissolves in water?

A

the molecules mix amongst eachother

56
Q
A

physics- D (3 decks)

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