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AP Chemistry > AP Chemistry Summer Assignment > Flashcards

AP Chemistry Summer Assignment Flashcards

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1
Q

The simplest form of matter

A

an element

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2
Q

Combinations of elements that have a definite composition

A

compounds

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3
Q

atoms of an element image

A

single dots

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4
Q

molecules of an element image

A

groups of two dots together

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5
Q

molecules of a compound image

A

groups of multiple dots together

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6
Q

elements/compounds existing in the solid state of matter…

A

definite shape, definite volume, particles are tightly packed and organized, particles vibrate gently in fixed positions

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7
Q

elements/compounds existing in the liquid state of matter…

A

indefinite shape (take shape of container), definite volume, particles are free to slide around one another

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8
Q

elements/compounds existing in the gas state of matter…

A

indefinite shape (takes shape of container), indefinite volume (spreads out to fill the space), particles are free to move around

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9
Q

all matter…

A

has mass and occupies space

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10
Q

physical properties

A

can be observed without changing the identity and composition of the substance

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11
Q

chemical properties

A

describe how a substance reacts with other substances

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12
Q

physical properties examples

A

color, odor, density, hardness, solubility, melting point, boiling point

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13
Q

chemical properties examples

A

acid-base reactions, oxidation and reduction (REDOX), and flammability

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14
Q

physical change

A

a substance changes its physical appearance, but not its composition

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15
Q

chemical change

A

also called a chemical reaction, a substance is transformed into a chemically different substance, often accompanied by observable changes like color changes and energy changes

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16
Q

physical change examples

A

most common are changes of state, solid to liquid (melting), liquid to gas (boiling), gas to liquid (condensing), solid to gas (sublimation), gas to solid (deposition), liquid to solid (freezing)

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17
Q

chemical change examples

A

Hydrogen (H2) burns in air (O2), chemical because it combines with oxygen to form water (H2O)

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18
Q

physical changes IMFs or IntraMFs

A

IMFs (the forces between particles) are disrupted, boiling water separates one water molecule (H2O) from another water molecule but does not break any individual water molecule apart

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19
Q

chemical changes IMFs or IntraMFs

A

Intramolecular forces (the forces within substances) are disrupted, during electrolysis of water, one water molecule (H2O) splits up to form O2 and H2 atoms, individual water molecules do break apart

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20
Q

which elements exist as diatomic molecules?

A

N, O, F, Cl, Br, I –> (start at 7 make a 7)

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21
Q

pulverise

A

to crush/grind

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22
Q

unit and symbol for Mass for SI (System International)

A

Kilogram, kg

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23
Q

unit and symbol for Length for SI (System International)

A

Meter, m

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24
Q

unit and symbol for Time for SI (System International)

A

Second, s

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25
Q

unit and symbol for amount of substance for SI (System International)

A

Mole, mol

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26
Q

unit and symbol for Temperature for SI (System International)

A

Kelvin, K

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27
Q

symbol and meaning for Giga for SI (System International)

A

G, 10⁹

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28
Q

symbol and meaning for Mega for SI (System International)

A

M, 10⁶

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29
Q

symbol and meaning for Kilo for SI (System International)

A

K, 10³

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30
Q

symbol and meaning for Deci for SI (System International)

A

d, 10⁻¹

31
Q

symbol and meaning for Centi for SI (System International)

A

c, 10⁻²

32
Q

symbol and meaning for Milli for SI (System International)

A

m, 10⁻³

33
Q

symbol and meaning for Micro for SI (System International)

A

µ, 10⁻⁶

34
Q

symbol and meaning for Nano for SI (System International)

A

n, 10⁻⁹

35
Q

symbol and meaning for Pico for SI (System International)

A

p, 10⁻¹²

36
Q

m to yd conversion

A

1.00m = 1.094yd

37
Q

mile to yd conversion

A

1.000 mile = 1760yd

38
Q

kg to lbs conversion

A

1.000kg = 2.205lbs

39
Q

in to cm conversion

A

1.00in = 2.54cm

40
Q

derived units

A

all other units can be derived from base quantities

41
Q

Volume

A

liters (L) or milliliters (mL), 000mL = 1.000 cm³, 1.00L = 1000. mL = 1000 cm³

42
Q

Density

A

the ratio of mass to volume, density=mass/volume, units could be g/L or g/cm³, etc.

43
Q

celsius to kelvin

A

temp in C + 273

44
Q

kelvin to celsius

A

temp in K - 273

45
Q

celsius to farenheit

A

(1.8(temp in C)) + 32

46
Q

farenheit to celsius

A

(temp in F - 32) / 1.8

47
Q

accuracy

A

how close a measurement is to the true value of the quantity that is measured

48
Q

precision

A

how closely two or more measurements of the same quantity are with one another

49
Q

Antoine Lavoisier

A

Law of Conservation of Mass: mass is neither created nor destroyed in a chemical reaction

50
Q

Joseph Proust

A

Law of Definite Proportion: the same compound always contains exactly the same proportion of elements by mass

51
Q

Dmitri Mendeleev

A

Periodic Table of Elements: first to conceive the modern Periodic Table of Elements, insisted certain spots of the table be left blank until the actual element in found that matched the predicted properties, this was done to preserve the elements with similar properties called groups or families

52
Q

John Dalton Law of Multiple Proportion

A

when two elements form a series of compounds, the ratios of the masses of the second element that combine with the first element can always be reduced to small whole numbers

53
Q

Dalton’s Atomic Theory

A
  1. all elements are made up of tiny particles called atoms, 2. the atoms of a particular element are identical, different elements have different kind of atoms, 3. atoms cannot be created or destroyed, 4. chemical compounds are formed when different kinds of atoms combine together, a particular compound always has the same relative numbers and types of atoms, 5. chemical reactions deal with the rearrangement of the atom, which changes the way they are combined together, there is no change to the atoms themselves in a chemical reaction
54
Q

Dalton’s Law of Partial Pressures

A

the total pressure exerted by a gaseous mixture is equal to the sum of partial pressures of each individual component in a gas mixture (Ptotal = PA + PB + PC +…)

55
Q

J.J. Thomson

A

he measured the charge to mass ratio of an electron using a Cathode Ray Tube

56
Q

Plum Pudding Model

A

J.J. Thomson, electrons are embedded in a cloud of protons

57
Q

Robert Milliken

A

Milliken Oil Drop Experiment, found the mass (9.11E-31 kg) and the charge (1.6E-19 C) of an electron when balancing the electric force and gravitational force an electron across a set of charged plates

58
Q

James Chadwick

A

discovered neutrons

59
Q

Ernest Rutherford

A

Nuclear Model, performed the famous Gold Foil experiment and proposed that the protons and neutrons are in the centre of an atom (nucleus) where the electrons fly around the nucleus, the nucleus is very small and the atom is mainly made of empty space

60
Q

Neil Bohr

A

Bohr Atomic Model, electrons are in specific orbits (energy level) around the nucleus and therefore electrons are quantized

61
Q

Quantum Mechanics Model

A

aka Electron Cloud Model, Neil Bohr helped develop, based on mathematical probabilities

62
Q

Aufbau Principle

A

formulated by Neil Bohr, the electrons fill orbitals starting at the lowest available energy states before filling higher states

63
Q

Max Planck

A

he proposed the light could be viewed as particles as well as waves

64
Q

Proton

A

+1 charge, 1 amu mass, in nucleus

65
Q

Neutron

A

0 charge, 1 amu mass, in nucleus

66
Q

Electron

A

-1 charge, 1/1836 amu mass, outside of nucleus

67
Q

Monoatomic anions

A

named by replacing the ending of the name of the element with -ide (example, H- = hydride ion)

68
Q

binary covalent compounds naming

A
  1. the name of the element farther to the left of the periodic table is usually written first (exception: oxygen is always written last), 2. if both elements are in the same group in the periodic table, the one having the higher atomic number is named first
69
Q

Greek prefixes

A

mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca

70
Q

Binary Acids

A

acids where hydrogen combines with a monoatomic anion, Hydro + (element stem)ic acid, example: Hydrochloric acid (HCl)

71
Q

-ate trick

A

group of 3 = XO3, Borate, Carbonate, Nitrate… group of 4 = XO4, Phosphate, Arsenate, Sulfate, Selenate… group of 3 = XO3, chlorate, bromate, iodate

72
Q

oxyanions name trend

A

Hypo - ite (-2 oxygens), -ite (-1 oxygen), -ate (base oxygen), per - ate (+1 oxygen)

73
Q

oxoanions

A

some contain hydrogen and are named accordingly: HPO₄²⁻ hydrogen phosphate

AP Chemistry (2 decks)

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