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Chemistry > Chapter 4-Electrons > Flashcards

Chapter 4-Electrons Flashcards

1
Q

electromagnetic radiation

A

a form of energy that exhibits wavelike behavior as it travels throughout space

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2
Q

electromagnetic spectrum

A

all the forms of electromagnetic radiation

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3
Q

what is the speed of light?

A

3.0x10^8 m/s

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4
Q

wavelength

A

the distance between corresponding points on adjacent waves

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5
Q

frequency

A

defined as the number of waves that pass a given point in a specific time, usually one second

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6
Q

electromagnetic radiation equation

A

c=λv
c= speed of light
λ= wavelength
v=frequency

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7
Q

λ and v are ________ proportional

A

inversely

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8
Q

thomas young

A

showed that light appeared to exhibit a wave nature through his double slit experiment

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9
Q

dual wave-particle nature

A

all EM radiation has both wavelike and particle like properties
particles also have wave-like properties

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10
Q

1 Hz=

A

1 wave/second

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11
Q

wavelength is ______ proportional to frequency

A

inversely

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12
Q

frequency is _______ proportional to energy

A

directly

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13
Q

wavelength is ________ proportional to energy

A

inversely

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14
Q

planck’s constant

A

6.626x10^-34 J x s

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15
Q

electrons in higher energy levels (further from the nucleus) have _______ energy

A

more

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16
Q

what happens when an electron falls from a high energy to a lower one?

A

it loses energy

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17
Q

if energy is added to an electron (if the electron is excited) what will it do?

A

move up an energy level

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18
Q

photon

A

a particle of electromagnetic radiation having zero mass and carrying a quantum of energy

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19
Q

ground state

A

the lowest energy state of an atom

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20
Q

excited state

A

a state in which an atom has a higher potential energy than it has in its ground state

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21
Q

photoelectric effect

A

the emission of electrons from a metal when light shines on the metal

22
Q

quantum of energy

A

the minimum quantity of energy that can be lost or gained by an atom

23
Q

Line emission spectrum

A

When a narrow beam of emitted light was shined through a prism, it was separated into the four specific colors of the visible spectrum

24
Q

Continuous spectrum

A

The emission of a continuous range of frequencies of electromagnetic radiation

25
Q

Emission

A

When an electron falls to a lower energy level and emits a photon

26
Q

Absorption

A

Energy added to an atom to move an electron to a higher energy level

27
Q

Heisenberg uncertainty principle

A

It is impossible to determine simultaneously both the position and the velocity of an electron or any other particle

28
Q

Quantum theory

A

Mathematically describes the wave properties of electrons and other particles

29
Q

Orbital

A

A three dimensional region around the uncles that indicates the probable location of an electron

30
Q

Quantum numbers

A

Specify the properties of atomic orbitals and the properties of electrons in orbitals

31
Q

Principle quantum number

A

Symbolized by n

Indicates the main energy level occupied by an electron

32
Q

Angular momentum quantum number

A

Symbolized by l

Indicates the shape of the orbital

33
Q

Magnetic quantum number

A

Symbolized by m

Indicates the orientation of an orbital around the nucleus

34
Q

Spin quantum number

A

Has only two possible values: +1/2, -1/2

Indicate the two fundamental spin states of an electron in an orbital

35
Q

Electron configuration

A

The arrangement if electrons in an atom

36
Q

Ground state electron configuration

A

Lowest energy arrangement of the electrons for each element

37
Q

Aufbau principle

A

An electron occupies the lowest energy orbital that can receive it

38
Q

Pauli exclusion principle

A

No two electrons in the same atom can have the same set of four quantum numbers

39
Q

Hund’s rule

A

Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin state

40
Q

Louis de broglie

A

Proposed that electrons, like light, also have a dual wave particle nature

41
Q

Emission spectra

A

Wavelengths of light that a substance emits when it’s electrons are excited

42
Q

Isoelectronic

A

Same electron configuration

43
Q

Valence electrons

A

Electrons found in outermost energy level of an atom

44
Q

S subshell

A

1 orbital

2 e- max

45
Q

P subshell

A

3 orbitals

6 e- max

46
Q

D subshell

A

5 orbitals

10 e- max

47
Q

F subshell

A

7 orbitals

14 e- max

48
Q

N=1

A 
One subshell (s)
2 e- max
49
Q

N=2

A 
Two subshells (s,p)
8 e- max
50
Q

N=3

A 
Three subshells (s,p,d)
18 e- max
51
Q

N=4

A 
Four subshells (s,p,d,f)
32 e- max

Chemistry (9 decks)

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