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AP Chemistry > Midterm > Flashcards

Midterm Flashcards

1
Q

Law vs. Theory

A

a law summarizes what happens, a theory is an attempt to explain why it happens

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2
Q

SI unit for mass

A

kg

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3
Q

SI unit for length

A

m

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4
Q

SI unit for electric current

A

ampere (A)

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5
Q

SI unit for luminous intensity

A

candela (cd)

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6
Q

Mega-

A

(M) 10^6

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7
Q

Pico-

A

(p) 10^-12

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8
Q

Micro-

A

10^-6

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9
Q

Nano-

A

(n) 10^-9

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10
Q

all mater is composed of extremely small particles called atoms

A

Dalton’s Atomic Theory

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11
Q

compounds have a constant composition by mass. they react in specific rations by mass.

A

Law of Definite Proportions

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12
Q

Discovered elections through the cathode ray tube experiment.

A

J. J. Thomson

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13
Q

Atoms of a given element are identical in sixe, mass, ad other properties

A

Dalton’s Atomic Theory

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14
Q

devised the Plum Pudding model

A

J. J. Thomson

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15
Q

atoms cannot be subdivided, created nor destroyed.

A

Dalton’s Atomic Theory

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16
Q

atoms of different elements can combine in simple whole-number rations to form chemical compounds

A

Dalton’s Atomic Theory

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17
Q

when two elements form more that one compound, the rations of the masses of the second element that combine with one gram of the first can be reduced to small whole numbers.

A

Law of Multiple Proportions

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18
Q

used the oil drop apparatus to determine the charge of an electron

A

Robert Millikan

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19
Q

in chemical reactions, atoms are combined, separated, or rearranged

A

Dalton’s Atomic Theory

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20
Q

discovered that the nucleus is small, dense, and positively charged through the gold foil experiment.

A

Rutherford

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21
Q

True or false: Protons and neutrons are fundamental particles.

A

False. they are made up of quarks
Protons: 2 ups, 1 down
Neutrons: 1 up, 2 downs

22
Q

What holds quarks together?

A

gluons

23
Q

Nitrate solubility

A

Always soluble

24
Q

Common strong acids

A

HCl, HBr, HI, HNO3, H2SO4, HClO4

25
Q

Common strong bases

A

Oxidized and hydroxides of I & II A metals

26
Q

Boyle’s Law

A

PV=PV

27
Q

Charles’ Law

A

V/T=V/T

28
Q

Avogadro’s Law

A

V/n=V/n

29
Q

Gay-Lussac Law

A

P/T=P/T

30
Q

1 Atm= _____ Pa

A

101,325

31
Q

The total pressure in a container is the sum of the pressure each was exert if it were alone in a container

A

Dalton’s law

32
Q

Particles are so small the we can ignore their volume

A

Kinetic molecular theory

33
Q

Root mean square equation

A

Maxwell equation

34
Q

[P+a(n/V)^2]x(V-nb)=nRT

A

Van dear Waal’s equation

35
Q

The particles do not affect each other, neither attracting nor repelling

A

Kinetic molecular theory

36
Q

Particles are in constant motion and their collisions carouse pressure

A

Kinetic molecular theory

37
Q

(r1/r2)=(M1/M2)^.5

A

Graham’s Law

38
Q

The average kinetic energy is proportional to the Kelvin temperature

A

Kinetic molecular theory

39
Q

Hess’s Law

A

Enthalpy of reaction = enthalpy of formation (products) - enthalpy of formation (reaction)

40
Q

Delta E = ?

A

q + w

41
Q

Work = ?

A

-P(delta T)

42
Q

Heat of solution

  • three steps
  • equation
A
  • 1) break intermolecular forces (+)
    2) disrupt IMF of water molecules (+)
    3) formation of ion-dipole forces (-)
  • above added together
43
Q

Electrons double-up while spinning in opposite directions

A

Pauli exclusion principle

44
Q

Electrons fill up hydrogen like orbitals from the lowest energy levels

A

Aufbau principle

45
Q

The lowest energy configuration for an atom is the one that has the maximum number of unpaired electrons.

A

Hund’s rule

46
Q

From %T to A

A

-log(%T/100) = A

47
Q

Beer’s Law

A

A=ecl
e= molecular absorbance
c= concentration
l= length of container

48
Q

Lattice energy equation:

E=(2.31x10^-19J•nm)(Q1Q2/r)

A

Coulomb’s Law

49
Q

Formal charge equation

A 
# valence e - # bonds - # lone electrons
* double bonds = 2 bonds
50
Q

Bond order equation for non diatomics.

A

bonds on central atom/# of free atoms on central atom.

AP Chemistry (3 decks)

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