Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chemistry > basic knowledge: must know > Flashcards

basic knowledge: must know Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

intermolecular forces vs intramolecular forces

A

intermolecular forces: between the molecules

intramolecular forces: between the atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

metallic intermolecular forces

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

ionic intermolecular forces

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

covalent intermolecular forces

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

polar covalent IF

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

nonpolar covalent IF

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

dipole-dipole interaction

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

hydrogen bonding

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

examples of nonpolar covalent bond.

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

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

A

isotope

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

isoelectronic radius increases as ________ increases

A

no. of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

polyatomic, transition metals cation

A

polyatomic: ium
transition: ous / ic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

monoatomic/polyatomic anion

A

ide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

oxyanions such as bromine, iodine, chlorine (BIC)

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

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

A

-ite, -ate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

other oxyanions end with

A

-ate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

when acid ends with:
ite:
ide:
ate:

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

in radioactive decay, these two properties are conserved

A

electric charge, and mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

types of radioactive decay:

A 
beta
alpha
positron
gamma
electron capture
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

beta decay

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

alpha decay

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

beta positron (electron but +)

A

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

25
Q

gamma decay

A

release of gamma radiation; no changes

26
Q

electron capture

A

nucleus reacts with the inner shell electron; converts p -> n thereby decreasing the atomic number

27
Q

quantum theory

A

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
Q

quantum number set

A

allowed energy states/levels of electrons

29
Q

four quantum numbers

A

principal
azimuthal
magnetic QN
magnetic spin

30
Q

principal QN

A

refers to the energy state/level; wherein n becomes bigger so does the atomic orbital

31
Q

responsible for the physical properties and chemical reactions of an atom; known as the excess EC at the outermost of the atom

A

valence electrons

32
Q

Atoms that are possible to have less/more than octet

A

Less than: Boron

More than: P, B, S, I (phosphate, bromine, sulfur, iodine)

33
Q

1 L is equivalent to what in grams?

A

1000g

34
Q

1 mole is equivalent to what in particles?

A

6.022 x 10^23 particles

35
Q

Molarity is dependent on the ??? while molality is independent

A

TEMPERATURE

36
Q

law of conservation of matter

A

the equations on both sides must be balanced to be equal

37
Q

theoretical value is the amount of products produced by the LR in grams; what is the actual value?

A

actual value is the real amount of products produced

38
Q

yield percent formula

A

actual products/theoretical products x 100

39
Q

1 atm = ____ torr = _____ mmHg = ______ kPa/Pa

A

760 torr/mmHg

101.325 kPa or 101325 Pa

40
Q

combined gas law

A

PV/nT = PV/nT

41
Q

charles law

A

P = V/T

42
Q

gay lussacs

A

V = P/T

43
Q

avogadros law

A

P&T=V/n

P&T = constant
n = moles
44
Q

value of K in ideal gas formula

A

0.0821 Lxatm/molxK

45
Q

ideal gas formula

A

PV=nRT

46
Q

derive density from ideal gas formula to get:

A

D = PM/RT

47
Q

What affects solubility?

A

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
Q

mole fraction

A

mole solute/total moles

49
Q

properties dependent on the number/amount of solute added, not on its kind (unlike intensive and extensive)

A

colligative properties

50
Q

what are the components of colligative properties?

A

vapor pressure, osmotic pressure, freezing and boiling point

51
Q

nonvolatile & nonelectrolyte solute + pure solvent

A

increased, osmotic pressure & boiling point

decreased vapor pressure and freezing point

52
Q

formula for BP

A

Delta T = Kb x m

Kb = constant; 0.512 C/m

53
Q

formula for FP

A

Delta T = Kt x m

Kt = 1.86 C/m

54
Q

formula for osmosis

A

osmosis = MRT

M = molarity (mol solute/ L solution)
R = 0.0821
T = kelvin
55
Q

nonvolatile electrolyte yung solute (read)

A

the effect on colligative properties is dependent on the number of ions formed

56
Q

3 concepts of acids and bases (BAL)

A

Arrhenius: presence of H and OH
Bronsted Lowry: protons
Lewis: electrons

57
Q

in bronsted lowry: the one that gives H+ _______

A

is an acid, once mabigay yung H - becomes conjugate base and vice versa

58
Q

polyprotic acids

A

where protons dissociate

59
Q

formula for acid-base titration

A

CV=CV

C = concentration in molarity/normality
V = volume in L or mL

chemistry (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions