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Gen Chem I - Exam #1 > Exam #1 > Flashcards

Exam #1 Flashcards

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1
Q

What defines an element?

A

the # of protons

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2
Q

Electrons

A
  • outside part of the atom
  • negative charge
  • effectively massless
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3
Q

Protons

A
  • inside the nucleus
  • positive charge
  • # determines identity of the element
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4
Q

changing # of neutrons

A

isotope

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5
Q

changing # of electrons

A

ion

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6
Q

changing # of protons

A

different element

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7
Q

Isotope Facts

A
  • named after the mass #
  • quantity vary among the elements
  • mass # in periodic table is the weighted average of isotope masses
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8
Q

Ions

A

the same element (same # of protons), different # of electrons, has a net electrical charge

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9
Q

Anions

A

when atoms GAIN electrons, overall negative charge

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10
Q

Cations

A

when atoms LOSE electrons, overall positive charge

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11
Q

How to find the # of electrons

A
  • if the net charge is 0, then the # of electrons = # of protons
  • if ion is positively charged, proton # - charge #
  • if ion is negatively charged, proton # + charge #
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12
Q

wavelength (λ)

A

the distance between corresponding points of a wave

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13
Q

frequency (u)

A

of wave cycles per unit time

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14
Q

What is the general relationship between frequency & wavelength?

A
  • as wavelength gets longer, frequency decreases
  • as wavelength gets shorter, frequency increases
  • INVERSELY RELATED
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15
Q

Relationship of Energy (E)

A
  • directly proportional to frequency
  • inversely proportional to wavelength
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16
Q

Reason for unique emission spectra for each element

A

the distinct arrangement and # of electrons in its atoms

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17
Q

Bohr Model of H Atoms

A
  • there are certain energy levels that an electron can occupy
  • the more energy levels fallen, the more energy emitted
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18
Q

Absorb

A

lower → higher

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19
Q

Emit

A

higher → lower

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20
Q

Problems with Bohr Theory

A
  • it only works for hydrogen
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21
Q

Bohr Theory was the first to…

A
  • indicate that electrons occupy various energy levels
  • indicate that electrons could transfer between energy levels
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22
Q

Location of metals

A

left side of periodic table

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23
Q

Location of metalloids

A

middle right of periodic table

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24
Q

Location of nonmetals

A

right side of periodic table, except hydrogen

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25
Q

Metal characteristics

A

ductile, conductive, shiny, malleable, all solid except mercury

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26
Q

Nonmetal characteristics

A

poor conductors of heat & electricity, brittle, can be all 3 states of matter

27
Q

Metalloid characteristics

A

typically appear shiny, brittle, semi conductors, good conductors

28
Q

Periods

A

horizontal rows, exhibit trends

29
Q

Groups

A

vertical columns, similar properties

30
Q

Group 1

A

Alkali Metals

31
Q

Group 2

A

Alkali Earth metals

32
Q

Group 3

A

Icosagens

33
Q

Group 4

A

Crystallogens

34
Q

Group 5

A

Phlctogens

35
Q

Group 6

A

Chalcogens

36
Q

Group 7

A

Halogens

37
Q

Group 8

A

Noble gases

38
Q

Alkali metal characteristics

A

soft, low melting points, low density, very reactive

39
Q

Alkali earth metal characteristics

A

harder, higher melting, denser than alkali metals, reactive but less than alkali metals

40
Q

Halogen characteristics

A

nonmetals, diatomic, F2 & Cl2 are gases, Br2 is liquid, I2 is solid, very reactive

41
Q

Noble gas characteristics

A

all gases are at room temp, very low melting & boiling points, very unreactive, lack strength

42
Q

Ionic

A

1 metal & 1 nonmetal, electrons are lost & gained to make ions which are then attracted to each other

43
Q

Covalent or Molecular

A

2 nonmetals, electrons are shared

44
Q

Wave particle duality

A

an electron can be described as both a particle & a wave

45
Q

Heisenberg Uncertainty Principle

A

we cannot know both the position & speed of a particle (such as a photon or electron) with perfect accuracy

46
Q

Determinancy

A

definite, can be precisely determined

47
Q

Indeterminacy

A

uncertain, cannot. be definitively known

48
Q

Orbits

A

fixed path where electrons revolve around the atom’s nucleus

49
Q

Orbitals

A

an area used to calculate the probability of finding any electron

50
Q

Schrödinger Equation

A

describes the form of probability waves, leads to quantum numbers

51
Q

Principle quantum number (n)

A

integer that determines overall size & energy for an orbital, L & mL are based on n

52
Q

Angular momentum quantum number (L)

A

determines the shape and name of the orbital

53
Q

Magnetic quantum number (mL)

A

determines orientation of orbital in space, mL is equal to the set of possible integers from -L to +L, # of solutions of mL are equal to the # of possible orientations of an orbital

54
Q

Spin Quantum number (mS)

A

determines the spin of the electron, not dependent on the other numbers, mS is either -1/2 or +1/2

55
Q

Pauli Exclusion Principle

A

no 2 electrons can have the same 4 quantum numbers

56
Q

Aufbau Principle

A

fill the lowest energy levels with electrons first

57
Q

Hund’s Rule

A

fill lower energy levels first singly with parallel spins

58
Q

Valence electrons

A
  • participate in chemical bonding
  • for main group elements (s & p orbitals)
  • outermost shell (principal energy levels)
59
Q

Core electrons

A
  • do NOT participate in chemical bonding
  • in complete principal energy level (previous noble gas)
  • in d & f orbitals
60
Q

dots in lewis dot structures represent…

A

valence electrons

61
Q

when are lewis dot structures useful?

A

when drawing covalent compounds

62
Q

how many electrons in each “box” of lewis dot structures?

A

2

63
Q

each line in a lewis dot structure represents…

A

a covalent bond

64
Q

guidelines for lewis dot structures for covalent compounds

A
  1. count total valence electrons
  2. create skeleton structure
  3. drawing single bonds to connect outer atoms to central atom
  4. check your work

Gen Chem I - Exam #1 (4 decks)

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