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Chemistry > Midterm Exam > Flashcards

Midterm Exam Flashcards

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1
Q

Chemical Properties

A

flammability, toxicity, reactivity, combustion, acidity

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2
Q

Physical Properties

A

density, color, hardness, reflectivity

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3
Q

chemistry

A

the branch of science that deals with the properties, composition, and structure of elements and compounds

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4
Q

Scientific Method

A
  1. observe
  2. state the problem
  3. form a hypothesis
  4. test hypothesis
  5. draw a conclusion
  6. communicate results
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5
Q

hypothesis

A

testable prediction

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6
Q

theories

A

generalizations made from many experiments

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7
Q

laws

A

generalizations that allow us to predict how things in nature will behave

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8
Q

SI Units

A

length: meter
mass: kilogram
time: second
temperature: kelvin
amount of a substance: mole
electric current: ampere
luminous intensity: candela

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9
Q

Dalton’s atomic theory

A
  1. all matter is composed of extremely small particles called atoms (wrong)
  2. atoms of a given element are identical in size, mass, and other properties (wrong)
  3. atoms cannot be subdivided, created, or destroyed (wrong)
  4. atoms of different elements combine in simple whole number ratios
  5. in chemical reactions, atoms are combined, separated, or rearranged
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10
Q

law of conservation of mass

A

matter cannot be created nor destroyed by normal means

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11
Q

law of conservation of energy

A

energy cannot be created nor destroyed but may be converted from one form to another

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12
Q

law of definite proportions

A

compounds are made up of the same ratio of elements no matter how much there is or where they are found

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13
Q

law of multiple proportions

A

if two or more compounds are composed of the same elements, then the ratio of the masses of the second elements combined with a certain mass of the first will always be small, whole numbers

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14
Q

Thomsons’ Cathode Ray Tube Conclusions

A
  1. electricity is composed of particles of matter (electrons)
  2. electrons are negatively charged
  3. electrons are very small
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15
Q

Oil Drop Conclusions

A
  1. mass of an electron is 1/2000 of a hydrogen atom
  2. same charge, but negative
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16
Q

Rutherford’s Gold Foil Conclusions

A
  1. the atom is composed of mostly empty space
  2. there is a small but very dense central core (nucleus)
  3. the nucleus has a positive charge
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17
Q

properties of neutrons

A
  1. about 1 amu
  2. neutral charge
  3. located in nucleus
18
Q

properties of protons

A
  1. about 1 amu
  2. positive charge
  3. located in nucleus
19
Q

properties of electrons

A
  1. about 1/2000 amu
  2. negative charge
  3. located in electron cloud
20
Q

atomic number

A

number of protons in an elements atom

21
Q

mass number

A

the sum of the protons and neutrons
(always whole numbers)

22
Q

Bohr Model

A
  1. electrons exist only in orbits with specific amounts of energy called energy levels
  2. electrons can only gain or lose certain amounts of energy
  3. only certain photons are produced
  4. energy of photons depends on the difference in energy levels
  5. each element has a unique bright-line emission spectrum
23
Q

Quantum Theory

A

Planck:
observed: emission of light from hot objects
concluded: energy is emitted in small, specific amounts (quanta)
quantum: minimum amount of energy change
Einstein:
observed: photoelectric effect
concluded: light has properties of both waves and particles

24
Q

Heisenberg Uncertainty Principle

A

impossible to know both the velocity and position of an electron at the same time

25
Q

Schrodinger Wave Equation

A
  1. finite number of solutions – quantized energy levels
  2. defines probability of finding an electron
26
Q

Principle quantum number

A

(n) – energy level
size of the orbital
n^2 – number of orbitals in the energy level

27
Q

Angular momentum quantum number

A

(l) – energy sublevel
shape of the orbital (s, p, d, f)

28
Q

Magnetic quantum number

A

(ml) – orientation of orbital
specifies the exact orbital within each sublevel
orbitals combine to form a spherical shape

29
Q

Spin quantum number

A

(ms) – electron spin (+1/2 or -1/2)
an orbital can hold two electrons that spin in opposite directions

30
Q

Aufbau Principle

A

electrons fill the lowest energy orbitals first

31
Q

Pauli Exclusion Principle

A

no two electrons in an atom can have the same 4 quantum numbers

32
Q

Hund’s rule

A

within a sublevel, place one electron per orbital before paring them

33
Q

Periodic law

A

when elements are arranged in order of increasing atomic number, elements with similar properties appear at regular intervals

34
Q

Ionic Bonds

A

form when electrons are transferred from a metal to a nonmetal

35
Q

Covalent Bonds

A

form as a result of two atoms sharing electrons

36
Q

Drawing Lewis Structures

A
  1. find total number of valence electrons
  2. arrange atoms – singular atom is usually in the middle
  3. form bonds between atoms
  4. distribute remaining electrons to give each atom an octet
  5. if there aren’t enough to go around make double / triple bonds
37
Q

Lattice Energy

A

amount of energy released when one mole of the substance forms from gaseous atoms

38
Q

VSEPR theory

A

valence shell electron pair repulsion theory
electron pairs orient themselves in order to minimize repulsive forces

39
Q

Chemical formulas

A
  1. what elements make up the compound (symbols)
  2. relative amounts (ratios) of each atom (subscripts)
40
Q

London Dispersion forces

A

attraction between two instantaneous dipoles

41
Q

dipole - dipole forces

A

attraction between two permanent dipoles
polar molecules

42
Q

hydrogen bonding

A

attraction between molecules with N-H, O-H, F-H bonds
extremely polar bonds

Chemistry (6 decks)

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