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basic knowledge: must know Flashcards

1
Q

intermolecular forces vs intramolecular forces

A

intermolecular forces: between the molecules

intramolecular forces: between the atoms

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2
Q

metallic intermolecular forces

A

sea of electrons; examples are gold and aluminum; good conductors; between metal to metal

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3
Q

ionic intermolecular forces

A

between metal and nonmetals; electrostatic attraction where cation donates - to anion; highest difference in electronegativity

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4
Q

covalent intermolecular forces

A

between nonmetal and nonmetal; they may share e equally or not

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5
Q

polar covalent IF

A

polar: electronegativity is between .5 to 2; unequal sharing of electrons

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6
Q

nonpolar covalent IF

A

equal sharing of electrons; similar electronegativity due to low difference such as less than 0.5

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7
Q

dipole-dipole interaction

A

partially charged + interacts with partially charged -; strongest attraction, interaction

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8
Q

hydrogen bonding

A

special type of dipole dipole, strong interaction/attraction, where H atoms react, bind with FON

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9
Q

london dispersion

A

neutral atom becomes dipole (turn into polarisable electron cloud) INCREASED polarizability if INCREASED electron cloud therefore INCREASED london dispersion; weakest and exists in all bonds, molecules

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10
Q

examples of nonpolar covalent bond.

A

h2o, oxygen, methane, ethane, nitrogen, hydrogen fluoride, hydrogen chloride

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11
Q

same element, same atomic number but different mass number or neutron number

A

isotope

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12
Q

isobar, isotone, isoelectronic

A

isobar: same mass number but different atomic number
isotone: same element, same neutrons
isoelectronic: same series, period and same no. of electrons

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13
Q

isoelectronic radius increases as ________ increases

A

no. of electrons

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14
Q

polyatomic, transition metals cation

A

polyatomic: ium
transition: ous / ic

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15
Q

monoatomic/polyatomic anion

A

ide

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16
Q

oxyanions such as bromine, iodine, chlorine (BIC)

A

O1: Hypo-, -ite
O2: -ite
O3: -ate
O4: Per-, -ate

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17
Q

oxyanions such as Samahan Ng Pokpok (sulfur, nitrogen, phosphate)

A

-ite, -ate

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18
Q

other oxyanions end with

A

-ate

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19
Q

when acid ends with:
ite:
ide:
ate:

A

ite: an-, -ous acid
ide: hydro-, -ic acid
ate: an-, -ic acid

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20
Q

in radioactive decay, these two properties are conserved

A

electric charge, and mass

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21
Q

types of radioactive decay:

A 
beta
alpha
positron
gamma
electron capture
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22
Q

beta decay

A

release of beta particles (fast speed electrons); convert n -> p thereby increasing atomic no.

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23
Q

alpha decay

A

release of alpha particles; releases 4 mass number and 2 atomic number (2 protons 2 neutrons)

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24
Q

beta positron (electron but +)

A

convert p -> n; same mass as electrons but diff. sign

25
gamma decay
release of gamma radiation; no changes
26
electron capture
nucleus reacts with the inner shell electron; converts p -> n thereby decreasing the atomic number
27
quantum theory
electrons at ground state becomes excited when reacts with a quanta (enough amount of energy) then goes back to being at ground state when light is emitted
28
quantum number set
allowed energy states/levels of electrons
29
four quantum numbers
principal azimuthal magnetic QN magnetic spin
30
principal QN
refers to the energy state/level; wherein n becomes bigger so does the atomic orbital
31
responsible for the physical properties and chemical reactions of an atom; known as the excess EC at the outermost of the atom
valence electrons
32
Atoms that are possible to have less/more than octet
Less than: Boron | More than: P, B, S, I (phosphate, bromine, sulfur, iodine)
33
1 L is equivalent to what in grams?
1000g
34
1 mole is equivalent to what in particles?
6.022 x 10^23 particles
35
Molarity is dependent on the ??? while molality is independent
TEMPERATURE
36
law of conservation of matter
the equations on both sides must be balanced to be equal
37
theoretical value is the amount of products produced by the LR in grams; what is the actual value?
actual value is the real amount of products produced
38
yield percent formula
actual products/theoretical products x 100
39
1 atm = ____ torr = _____ mmHg = ______ kPa/Pa
760 torr/mmHg | 101.325 kPa or 101325 Pa
40
combined gas law
PV/nT = PV/nT
41
charles law
P = V/T
42
gay lussacs
V = P/T
43
avogadros law
P&T=V/n ``` P&T = constant n = moles ```
44
value of K in ideal gas formula
0.0821 Lxatm/molxK
45
ideal gas formula
PV=nRT
46
derive density from ideal gas formula to get:
D = PM/RT
47
What affects solubility?
nature of solvent and solute temperature: in solid to liq (temp increases with solubility); in gases (sol decreases when temp increases) pressure (only works with gases or vaporization; higher pressure = higher solubility of liquid-gas)
48
mole fraction
mole solute/total moles
49
properties dependent on the number/amount of solute added, not on its kind (unlike intensive and extensive)
colligative properties
50
what are the components of colligative properties?
vapor pressure, osmotic pressure, freezing and boiling point
51
nonvolatile & nonelectrolyte solute + pure solvent
increased, osmotic pressure & boiling point | decreased vapor pressure and freezing point
52
formula for BP
Delta T = Kb x m Kb = constant; 0.512 C/m
53
formula for FP
Delta T = Kt x m Kt = 1.86 C/m
54
formula for osmosis
osmosis = MRT ``` M = molarity (mol solute/ L solution) R = 0.0821 T = kelvin ```
55
nonvolatile electrolyte yung solute (read)
the effect on colligative properties is dependent on the number of ions formed
56
3 concepts of acids and bases (BAL)
Arrhenius: presence of H and OH Bronsted Lowry: protons Lewis: electrons
57
in bronsted lowry: the one that gives H+ _______
is an acid, once mabigay yung H - becomes conjugate base and vice versa
58
polyprotic acids
where protons dissociate
59
formula for acid-base titration
CV=CV ``` C = concentration in molarity/normality V = volume in L or mL ```

chemistry (7 decks)

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