Chapter 4 Flashcards

1
Q

electromagnetic radiation

A

a form of energy that exhibits wave light behavior as it travels through space

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2
Q

electromagnetic spectrum

A

all forms of electromagnetic radiation

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3
Q

wavelength

A

the distance between corresponding points on adjacent waves.

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4
Q

Frequency

A

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

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5
Q

photoelectric effect

A

refers to the emission of electrons from a metal when light shines on the metal.

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6
Q

Quuantum

A

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

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7
Q

photon

A

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

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8
Q

Ground State

A

lowest energy state of an atom.

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9
Q

excited state

A

when a atom has a higher potential energy than its ground state

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10
Q

line-emission spetrum

A

specific frequencies emitted by the element.

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11
Q

continuous spectrum

A

emission of a continuous range of frequencies of electromagnetic radiation

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12
Q

Heisenberg uncertainty principle

A

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

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13
Q

Quantum theory

A

describes mathematically the wave properties of electrons and other very small particles.

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14
Q

orbital

A

a three dimensional region around the nucleus that indicates the probable location of an electron.

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15
Q

Quantum numbers

A

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

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16
Q

Principal quantum numbers

A

symbolized by “n” indicates the main energy level occupied by the electron

17
Q

Angular momentum quantum number

A

symbolized by ‘l’ indicates the shape of an orbital

18
Q

manetic quantum number

A

symbolized by ‘m’indicates the orientation of an orbital around the nucleus.

19
Q

Spin quantum number

A

only 2 possible values (+1/2, -1/2) indicates the 2 fundamental spin states of an electron in an orbital.

20
Q

electron configuration

A

the arrangement of electrons in an atom

21
Q

aufbau principle

A

an electron occupies the lowest energy orbital that can receive it.

22
Q

Pauli extension principle

A

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

23
Q

Hund’s rule

A

orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron

24
Q

highest occupied level

A

the electron containing main energy level with the highest principal quantum number.

25
inner-shell electron
electrons that are not in the highest occupied energy level.
26
noble gases
the group 18 elements
27
noble gas configuration
the electron configuration of a noble gas