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CAPP Chemistry > Chapter 3 > Flashcards

Chapter 3 Flashcards

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1
Q

Speed of Light (c)

A

2.998x10^8 m/s

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2
Q

Wavelength (λ)

A

distance between two consecutive peaks or troughs in a wave

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3
Q

Frequency (v)

A

number of successive wavelengths that pass a given point in a unit of time

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4
Q

Amplitude

A

one-half the distance between the peaks and troughs

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5
Q

Unit for Frequency

A

hertz (Hz)

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6
Q

MHz –> Hz

A

1 –> 10^6

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7
Q

GHz –> Hz

A

1 –> 10^9

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8
Q

Speed of the Wave

A

λv

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9
Q

As the wavelength increases, the frequency…

A

decreases

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10
Q

As the frequency increases, the wavelength…

A

decreases

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11
Q

Planck’s Number (h)

A

6.626x10^-34 Js

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12
Q

E=

A

hv

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13
Q

v=

A

c/λ

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14
Q

Ground State (of an atom)

A

occurs when the electron is in the lowest energy orbit (n=1)

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15
Q

Excited State (of an atom)

A

occurs when it is possible for the electron to move to an orbit with a higher n-value, which has higher energy

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16
Q

An atom absorbs energy and the electron moves…

A

from a lower n to a higher n

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17
Q

An atom emits energy and the electron moves…

A

from a lower n to a higher n

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18
Q

Energy of Electron Orbital Movement (equation)

A

ΔE=k{[1/(n1)^2]-[1/(n2)^2]}

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19
Q

k=

A

2.179x10^-18 J

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20
Q

Principal Quantum Number or Shell Number

A

n

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21
Q

Angular Momentum Quantum Number

A

l

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22
Q

For l=0

A

s orbital

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23
Q

For l=1

A

p orbital

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24
Q

For l=2

A

d orbital

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25
Q

For l=3

A

f orbital

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26
Q

of Possible S Orbital Shapes

A

1

27
Q

of Possible P Orbital Shapes

A

3

28
Q

of Possible D Orbital Shapes

A

5

29
Q

of Possible F Orbital Shapes

A

7

30
Q

Magnetic Quantum Number

A

m

31
Q

Spin Quantum Number

A

ms

32
Q

ms=

A

1/2 or -1/2

33
Q

Pauli Exclusion Principle

A

no two electrons in the same atom can have exactly the same set of all four quantum numbers

34
Q

Subshell Electron Capacity (low —> high E)

A

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

35
Q

Aufbau Principle

A

Add the number of electrons equal to the atomic number one at a time to the subshell of the lowest available energy

36
Q

Core Electrons

A

electrons occupying the inner shell orbitals

37
Q

Valence Electrons

A

electrons occupying the orbital(s) in the outermost shell (highest value of n)

38
Q

Electron Configuration of Cu

A

[Ar] 4s1 3d10

39
Q

Electron Configuration of Cr

A

[Ar] 4s1 3d5

40
Q

Periodic Trend (size or radius)

A

increase down a group and decreases across a period

41
Q

A cation is always ___ than the atom from which it is derived

A

smaller

42
Q

A anion is always ___ than the atom from which it is derived

A

larger

43
Q

Isoelectronic

A

atoms and ions that have the same electron configuration

44
Q

Periodic Trend (ionization energy)

A

amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state

decreases down a group, increases across a period

45
Q

Be (4) has a ___ IE than B (5)

A

higher

46
Q

O (8) has a ___ IE than N (7)

A

lower

47
Q

removing an electron from a CATION is ___ than removing an electron from a neutral atom

A

harder

48
Q

Electron Affinity (EA)

A

the energy change for the process of adding an electron to a gaseous atom to form an ANION

49
Q

A negative EA means…

A

energy is released (exothermic)

50
Q

A positive EA means…

A

energy is required (endothermic)

51
Q

Periodic Trends (electron affinities)

A

more negative EA across a period

52
Q

Deviations to EA Trend

A

group 18 (filled shell), group 2 (filled ns subshell), group 15 (half-filled np subshell)

53
Q

Metals (left)

A

shiny, malleable, good conductors of heat and electricity

54
Q

Nonmetals (right)

A

appear dull, poor conductors of heat and electricity

55
Q

Metalloids (touching staircase - Al)

A

conduct heat and electricity moderately well, possess some properties of metals and some properties of nonmetals

56
Q

Group 1 (except hydrogen)

A

alkali metals

57
Q

Group 2

A

alkaline earth metals

58
Q

Group 17

A

halogens

59
Q

Group 18

A

noble or inert gases

60
Q

Ionic Bonds

A

electrostatic forces of attraction caused by the transferring of electrons

  • metals form cations
  • nonmetals create anions
61
Q

Covalent Bonds

A

caused when electrons are shared between two nonmetals

62
Q

Properties of Ionic Compounds

A
  • solids typically have higher melting and boiling points
  • nonconductive in solid form
  • conductive in molten form
63
Q

Properties of Covalent Bonds

A
  • often exist as gases
  • have low boiling points as liquids
  • low melting points as solids

CAPP Chemistry (8 decks)

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