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Chemistry Flashcards

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1
Q

atomic model; the atom is hard and indestructible

A

Billiard Ball Model (John Dalton)

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2
Q

atomic model; electrons are embedded in a positively-charged sphere

A

Plum Pudding Model (JJ Thompson)

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3
Q

atomic model; the mass and all of the positive charge of an atom are concentrated on the nucleus

A

Nucleus Model (Ernest Rutherford)

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4
Q

atomic model; electrons travel around the nucleus in a circular orbit; their energy is proportional to their distance from the nucleus

A

Planetary Model (Niels Bohr)

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5
Q

atomic model; the electron is a wave (found in orbitals)

A

Quantum Model

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6
Q

5 atomic models

A
  • Billiard Ball
  • Plum Pudding
  • Nuclear
  • Planetary/Bohr
  • Quantum
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7
Q

number of protons in the nucleus; also equal to the number of electrons

A

atomic number

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8
Q

protons + neutrons

A

mass number

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9
Q

True or False: in an atom, the number of protons is constant

A

True

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10
Q

The Atomic Theory

A
  • all matter are made up of atoms
  • all atoms of an element have identical chemical and physical properties
  • atoms of different elements have different sets of chemical and physical properties
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11
Q

atoms of the same element that differ in the number of neutrons

A

isotopes

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12
Q

highly reactive metals

A

alkali metals

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13
Q

highly reactive non-metals

A

halogens

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14
Q

inert gases, highly stable elements

A

noble gases

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15
Q

charged atom

A

ion

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16
Q

negatively charged ion; gain in electrons

A

anion

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17
Q

positively charged ion; loss in electrons

A

cation

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18
Q

energy required to remove an electron from an atom

A

ionization energy

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19
Q

energy released when an electron is added to an atom

A

electron affinity

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20
Q

ability to attract electrons

A

electronegativity

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21
Q

4 Quantum numbers

A
  • principal
  • azimuthal
  • magnetic
  • spin
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22
Q

the number of excess electrons of an atom

A

valence electrons

23
Q

every element has the same electronic configuration as the element before it in the periodic table, plus one extra

A

Aufbau Principle

24
Q

electrons tend to stay unpaired in orbitals with equal energies

A

Hund’s Rule

25
Q

Phases of Matter

A
  • Solid
  • Liquid
  • Gas
26
Q

3 types of Mixture

A
  • solution
  • colloid
  • suspension
27
Q

type of solution that can still dissolve more solute

A

unsaturated

28
Q

type of solution that already contains the maximum amount of sollute

A

saturated

29
Q

type of solution that used pressure or heat to dissolve more than the usual amount of sollute

A

supersaturated

30
Q

6 Gas Laws

A
  • Boyle’s
  • Charles’
  • Gay-Lussac’s
  • Combined
  • Avogadro’s
  • Ideal
31
Q

P1V1= P2V2

A

Boyle’s

32
Q

V1/T1 = V2/T2

A

Charles’

33
Q

P1VI/T1= P2V2/T2

A

Combined

34
Q

VI/n1 = V2/n2

A

Avogadro’s

35
Q

pV = nRT

A

Ideal

36
Q

Kinetic Molecular Theory of Gases

A
  1. particles are infinitely small
  2. in constant random motion
  3. elastic collisions
  4. do not experience intermolecular force
  5. kinetic energy are directly proportional to their temperatures
37
Q

mass of reactants = mass of products

A

law of conservation of mass

38
Q

ratio of elements are always the same

A

law of definite proportion/composition

39
Q

weight of one mole of a material

A

molar mass

40
Q

avogadro’s number

A

1 mole = 6.02x10^23

41
Q
A
42
Q

the chemical formula in lowest

A

emirical formula

43
Q

Laws of Thermodynamics

A
  1. Law of Conservation of Energy - energy can neither be reated nor destroyed. it can only change forms.
  2. Entropy - degree of disorder
  3. entropy at absolute zero is zero
44
Q

amount of energy needed to raise the temperature of a substance by one degree

A

specific heat

45
Q

hotness or coldness

A

temperature

46
Q

total kinetic energy of molecules

A

heat

47
Q

heat lost or gained during a change in temperature

A

sensible heat

48
Q

heat lost or gained during a phase change

A

latent heat

49
Q

factors that increase rates of reaction

A
  • higher temperature
  • higher concentration of reactants
  • large surface area
    catlyst
50
Q

transfer electrons

A

ionic compound

51
Q

sharing of electrons

A

covalent compund

52
Q

comparative strengths of chemical bonding

A

ionic > covalent > hydrogen > dipole-dipole forces > London dispersion

53
Q
A

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