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Chemistry Fall Final > chemistry > Flashcards

chemistry Flashcards

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1
Q

Physical Change

A

Physical changes occur when matter changes its property (shape or size) ex: dissolves, changes phase (solid/liquid/gas)

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2
Q

Chemical Change

A

Chemical changes occur when matter becomes a new or different matter ex: gas production, color change, light production, precipitate production (two liquids together to form a solid)

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3
Q

4 States of Matter

A

solid, liquid, gas, plasma

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4
Q

Kinetic Theory of Matter

A

Matter is made up of atoms which are continual in a random motion

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5
Q

Element

A
  • consist of only one type of atom - cannot be further broken down into simple substance by any chemical or physical means ex: H (hydrogen)
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6
Q

Compound

A
  • pure substances - made up of more than one element - can be decomposed by chemical means - electrically neutral - fixed ratio ex: H20 (water)
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7
Q

Mixture

A
  • two or more pure substances together without reacting with each other - not chemically bonded - not in fixed ratio
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8
Q

Homogeneous Mixture

A
  • uniform distribution - evenly spread out and look the same ex: sugar & water
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9
Q

Filtration

A
  • the process of filtering a liquid, especially with water - when water is poured through a filter, any undissolved particles inside the water are left behind in the filter * used to separate heterogeneous mixture
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10
Q

Heterogeneous Mixture

A
  • things look different - not evenly mixed ex: sand & water
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11
Q

Distiliaton

A
  • the separation of one substance from another by evaporation and condensation - uses difference in boiling points ex: alcohol & water
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12
Q

Crystallization/Evaporation

A

the separation of solid from liquid by evaporation ex: sugar & water

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13
Q

Heat Transfer

A

the heat transferred is proportional to the mass of the object, the specific heat capacity of the object and the temperature change the object undergoes

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14
Q

Heat of Fusion

A
  • the energy required to change 1 gram of a substance from the solid to the liquid state without changing its temperature - fusion –> melting
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15
Q

Heat of Vaporation

A

the energy required to change 1 gram of a substance from the liquid to the gas state without changing its temperature

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16
Q

What happens when heat is absorbed or released?

A
  • temperature changes - phase changes (no temperature changes)
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17
Q

Vapor Pressure

A
  • the pressure exerted by a vapor in equilibrium with its liquid state - vapor pressure increases with increasing temperature - as temperature increases, the amount of vapor generated by a liquid in a closed container increases
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18
Q

Boiling

A
  • boiling occurs when the vapor pressure above the liquid equals the atmospheric pressure - boiling points change when pressure changes
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19
Q

Inter-molecular Force

A

attraction or bond between molecules

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20
Q

Liquids with strong inter-molecular force have…

A

a high boiling point

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21
Q

Materials with strong inter-molecular forces have…

A

low vapor pressure & high boiling point

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22
Q

When does a real gas behave like an ideal gas?

A

low pressure & high temperature ex: hydrogen & helium

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23
Q

Real Gas

A

attractive forces & volume

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24
Q

Ideal Gas

A

no attractive forces & no volume

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25
Q

Boyle’s Law

A
  • as pressure on a gas increases in a closed container, the volume of the gas decreases - pressure and volume are indirectly related
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26
Q

Gay-Lussac’s Law

A
  • at constant volume, an increase in temperature causes the pressure to increase - pressure and temperature are directly related
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27
Q

Charles’ Law

A
  • at constant pressure, an increase in temperature causes the volume to increase - volume and temperature are directly related
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28
Q

Avogadro’s Law

A

when the volume, temperature and pressure of two gases are the same, they contain the same number of molecules

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29
Q

Democritus’ Atomic Theory

A

the smallest piece of matter is “Atomos” (the atom)

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30
Q

Dalton’s Atomic Theory

A
  • first testable “atomic theory” - all elements are composed of indivisible, indestructible, and unchangeable atoms - atoms of the same element are identical (masses) & vice-versa - compounds are formed when atoms of two or more elements join together, in a fixed ratio
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31
Q

Thomson’s Atomic Theory

A
  • passed electric current through a neutral gas - electrons are much smaller than atoms and part of all atoms - plum pudding model
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32
Q

Rutherford’s Atomic Theory

A
  • most of the mass is in a tiny, positively charged nucleus - most of the atom’s volume is empty space - electrons exist in the space around the nucleus - gold foil experiment: shot alpha particles at a thin foil, most particles went straight through, but some were reflected back
33
Q

Chadwick’s Atomic Theory

A
  • the mass of protons is less than the actual mass of the nucleus - the discovery of the nucleus
34
Q

Bohr’s Atomic Theory

A
  • electrons orbiting the nucleus only exist in certain energy levels - electron shells can hold a fixed number of electrons - only electrons in the outermost shell take place in chemical reactions
35
Q

The Wave-Mechanical Model

A

according to the theory of wave mechanics, electrons do not move about an atom in a definite path

36
Q

Electron Cloud

A
  • a.k.a orbital - a space in which electrons are most likely to be found
37
Q

Atomic Spectra

A
  • when electrons gain energy they go from the ground state to the excited state - when they return to the ground state, they release light energy in different colors
38
Q

Atomic Number

A

shows the number of protons in an atom

39
Q

Mass Number

A

shows the number of protons and neutrons in an atom

40
Q

Number of Electrons

A

of electrons = # of protons

41
Q

Ions

A
  • an element whose number of protons is not equal to the number of electrons - the number of protons remains the same while the number of electrons changes
42
Q

Valence Electrons

A
  • atoms with the same number of protons, but different numbers of neutrons - atoms of the same element with different mass numbers
43
Q

Atomic Mass

A
  • the weighted average mass of all the atomic masses of the isotopes of that atom

Mass of isotope 1 (%) Mass of isotope 2(%)

_________________ + __________________

         100                                                    100
44
Q

Alpha Particles

A
  • Atomic mass: 4
  • Charge: 2+
  • Symbol: 42He
45
Q

Beta Particles

A
  • Composition: beta particles, same as electrons
  • Symbol: ß- or 0-1e
  • Charge: -1
  • Mass Number: 0
46
Q

Positron Particles

A
  • Composition: same as an electron, except +1
  • Symbol: ß+ or +10e
  • Mass: 0
  • Charge: +1
47
Q

Gamma Decay

A
  • Symbol: V
  • Charge: 0
  • Mass Number: 0
  • Does not affect mass number of atomic number
48
Q

Half-Life

A
  • the time taken for half of the radioactive atoms in a sample to decay
  • time elapsed/half-life
49
Q

Transmutation

A
  • a change in the nucleus of an atom that converts it from one element to another
50
Q

Natural Transmutation

A

when a transmutation occurs naturally

51
Q

Atrificial Transmutation

A

the bombardment of the nucleus by high-energy particles

52
Q

Fission

A
  • splitting of a heavy nucleus to produce lighter nuclei
  • begins by capturing a neutron
53
Q

Fusion

A
  • combining two small atoms to produce a heavier atom
  • high temperature and high pressure are required for fusion reaction
54
Q

Carbon Dating

A

Use of the isotopes C-14 & C-12 to find out the ages of organisms

55
Q

In both fission and fusion, the total mass the products is…

A

less than the total mass of the reactants

Products < Reactants

56
Q

Groups on the Periodic Table

A
  • elements in the same group have the same number of valence electrons
  • similar chemical properties
57
Q

Periods on the Periodic Table

A

elements in the same period have the same number of orbits/shells

58
Q

Group 1 of the Periodic Table

A

Alkali metals

59
Q

Group 2 of the Periodic Table

A

Alkaline earth metals

60
Q

Group 17 of the Periodic Table

A

Halogens

61
Q

Group 18 of the Periodic Table

A

Noble gases

62
Q

Groups 3 to 12 of the Periodic Table

A

Transition metals

63
Q

Properties of Metals

A
  • maleable & ductile
  • shiny
  • conducts electricity
  • high melting point & highly dense
  • lose electrons & form positive charges called cations
  • solids at STP (except mercury)
64
Q

Non-Metals

A
  • brittle & non-ductile
  • dull
  • does not conduct electricity
  • low melting point & less dense
  • gain electrons & form negative charges, called anions
  • can be solids, liquids or gases
65
Q

Metalloids

A
  • atoms that gain or lose electrons and forms ions when bonding
  • have properties of metals and non-metals
  • can be located using the “staircase”
66
Q

Electronegativity

A
  • the ability to attract electrons
  • non-electrons attract electrons more
  • Non-metals have higher electronegativty than metals
67
Q

Ionization Energy

A
  • the amount of energy needed to remove one (the outermost) electron from an atom
  • ionization energy for non-metals
68
Q

Noble Gases

A
  • group 18 elements
  • stable, do not react with other gases
  • a.k.a. inert gases
69
Q

Ionic Bond Formation

A
  • electron(s) are transferred from the metal atom to the non-metal atom
  • metals lose electrons and form positive charge and non-metals gain electrons and form negative charge
70
Q

Covalent Bond

A
  • between non-metal and non-metal
  • formed by sharing electrons
71
Q

Molecular Compounds

A

the compounds with covalent bonds

72
Q

Polar Covalent Bond

A
  • electrons are shared unequally
  • the difference in electronegativity is between 1.7 and 0.5
73
Q

Non-Polar Covalent Bond

A
  • electrons are shared equally
  • the difference in electronegativity is between 0.4 and 0
74
Q

Symmetrical Compounds

A
  • some compounds can be non-polar even though the bond present in them is polar
  • those compounds are symmetrical, equal distribution of charge
75
Q

Hydrogen Bond

A
  • a type of strong inter-molecular force
  • bond between: H&F, H&O, H&N ***FON***
76
Q

Properties of an Ionic Bond

A
  • does not conduct electricity in solid state
  • conducts electricity in solution (water)
  • soluble in water
  • high melting and boiling point
77
Q

Properties of a Covalent Bond

A
  • does not conduct electricity in solid state
  • does not conduct electricity in solution (water)
  • less soluble in water
  • low melting and boiling point
78
Q

Metallic Bond

A
  • found between metals and metals
  • the valence electrons can mover freely, and so each electron becomes detached from its parents atom
  • the electrons are said to be delocalized
  • metals conduct electricity in their solid states
79
Q

Polyatomic Ions

A
  • made up of more than one atom
  • polyatomic atoms are always in parenthesis, with the charges outside

Chemistry Fall Final (1 decks)

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