Chapter 6: Electronic Structure of Atoms

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19 Terms

1

Electronic Structure

The arrangement and energy of electrons.

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2

Wavelength (\lambda)

The distance between corresponding points on adjacent waves.

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3

Frequency (v)

The number of waves passing a given point per unit of time.

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4

Speed of Light (c)

The speed at which all electromagnetic radiation travels, approximately 3.00\cdot 10^{8}m/s

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5

Photoelectric Effect

The phenomenon where electrons are ejected from a metal when it absorbs energy that is proportional to frequency.

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6

Plank’s Constant ($h$)

A constant valued at 6.626\cdot 10^{-34}J\cdot s used in the photoelectric effect equation (E=hv).

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7

Quantum Mechanics

The branch of physics that describes the movement and behavior of electrons.

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8

Principal Quantum Number (n)

Describes the energy level of an orbital and is an integer greater than or equal to 1.

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9

Angular Momentum Quantum Number (l)

Defines the shape of the orbital, with allowed values ranging from 0 to n-1.

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10

Magnetic Quantum Number (m_l)

Describes the three-dimensional orientation of the orbital with allowed values from -l to l.

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11

Hund’s Rule

For orbitals in the same sublevel, each must contain one electron before any pairing occurs.

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12

Pauli Exclusion Principle

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

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13

Electron Configuration

The distribution of electrons in an atom, specified by energy level, orbital type, and number of electrons.

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14

Ground State

The lowest possible energy configuration of an atom's electrons.

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15

Condensed Electron Configuration

A shorthand notation for electron showing valence electrons and using noble gas symbols.

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16

s Orbitals

Spherical-shaped orbitals with a value of l equal to 0.

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17

p Orbitals

Orbital shape with two lobes and one nodal plane, with a value of l equal to 1.

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18

d Orbitals

Orbitals with more complex shapes, where the value of l is 2.

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19

f Orbitals

Highly complex-shape orbitals with a value of l equal to 3.

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