Chapter 11 Flashcards

0
Q

Length of a wave (measured in nm); the distance between peaks

A

Wavelength (T)

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1
Q

Energy transmitted from one place to another by light in the form of waves

A

Electromagnetic radiation

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2
Q

The vertical distance from the middle of the wave to the crest/trough

A

Amplitude

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3
Q

The top of a wave

A

Peak/crest

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4
Q

The number of waves that pass through a specific point in a given amount of time (measured in waves/sec or hertz (Hz)

A

Frequency (V)

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5
Q

Waves of electromagnetic radiation from short to long

A

Gamma rays, x-rays, ultraviolet, visible light, infrared, microwaves, radio waves

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6
Q

Light shining on a metal emits electrons

A

Photoelectric effect

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7
Q

Packets of light (quantum); particles of electromagnetic radiation (have no mass)

A

Photons

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8
Q

Planck’s equation

A

E=h•V

H= 6.626•10^-34

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9
Q

Speed of light equation

A

C=T•V

C=3.0•10^8

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10
Q

Rainbow colors within a given range

A

Continuous spectrum (visible spectrum)

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11
Q

Consists of several distinct lines of color each with its own frequency; each element has one

A

Bright line spectrum (line emission spectrum)

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12
Q

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

A

Quantum

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13
Q

Lowest energy state

A

Ground state

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14
Q

Atom has higher potential energy than at ground state

A

Excited state

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15
Q

Describes mathematically the wave properties of electrons and other very small particles

A

Quantum Theory

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16
Q

Properties of orbitals and electrons in the orbitals

A

Quantum numbers

17
Q

3-D place around the nucleus that indicates the probable location of an electron

18
Q

Main energy level occupied by an electron; as it increases so does electrons energy and distance (1-7)

A

Principle quantum number (n)

19
Q

Sublevels (l) indicate the shape of the orbital (s,p,d,f)

A

Angular momentum quantum number

20
Q

Orientation of an orbital around a nucleus

A

Magnetic quantum number

21
Q

Two values (Clockwise or counterclockwise)

A

Spin quantum number

22
Q

Arrangement of electrons in an atom

A

Electron configuration

23
Q

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

A

Heisenberg principle

24
An electron occupies the lowest energy level that can receive it
Aufbau principle
25
No two electrons in the same atom can have the same set of four quantum numbers
Pauli exclusion principle
26
Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron; all electrons in singly occupied orbitals have the same spin
Hund's rule
27
Electron containing main energy level with highest principle quantum number
Highest occupied level
28
Not in highest energy level
Inner shell electrons
29
N=______ N^2=______ 2N^2=______
Energy level Number of orbitals on that energy level Number of total electrons on that energy level
30
Electrons in the outermost s and p orbitals
Valence electrons
31
5-10 rule
Chromium and copper
32
The energy required to remove one outer electron from an atom
Ionization energy
33
The distance from the nucleus to the outer electron shell
Atomic radius
34
Energy associated with an atom gaining an electron
Electron affinity
35
A number that describes the relative ability of an atom (when bonded) to attract electrons
Electronegativity
36
__________decreases from left to right and increases from top to bottom
Atomic radius
37
__________increases from left to right and decreases from top to bottom
Ionization energy, electron affinity, and electronegativity
38
Nonmetal reactivity ______ from top to bottom
Decreases
39
Metal reactivity ______ from top to bottom
Increases
40
The left side of the electromagnetic radiation spectrum has ____ wavelength, ____ frequency, and ____ energy while the right side has ____ wavelength, ____ frequency, and ____ energy
``` Short High High Long Low Low ```