Unit Two: Structure and Properties

Question 1

Emission Spectrum

Answer 1

A characteristic spectrum of distinct, coloured lines that result when excited atoms emit light: can be observed through a spectroscope or a diffraction grating when a high voltage is passed through a gas in a gas tube.

Question 2

Absorption Spectrum

Answer 2

The spectrum that is produced when electrons of atoms absorb photons of certain wavelengths, causing the electrons to be excited from lower energy levels to higher energy levels.

Question 3

Orbitals

Answer 3

Solved wave functions that describe a region of probable location of electrons.

Question 4

Quantum Mechanical Model of the Atom

Answer 4

A model that describes atoms as having certain allowed quantities of energy because of the wave-like properties of their electrons.

Question 5

Ground State

Answer 5

The most stable energy state.

Question 6

Principal Quantum Number (n)

Answer 6

A positive whole number (integer) that indicates the energy level and relative size of an atomic orbital.

Question 7

Magnetic Quantum Number (m1)

Answer 7

An integer that indicates the orientation of an orbital in the space around the nucleus; values range from -1 to +1, including 0.

Question 8

Pauli Exclusion Principle

Answer 8

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Question 9

Spin Quantum Number (ms)

Answer 9

The quantum number that specifies the direction in which the electron is spinning with values of +1/2 and -1/3.

Question 10

Electron Configuration

Answer 10

A shorthand notation that shows the number and arrangement of electrons in an atom’s orbitals.

Question 11

Aufbau Principle

Answer 11

The principle behind an imaginary process of building up the electron structure of the atoms, in order of atomic number.

Question 12

Orbital Diagram

Answer 12

A diagram that uses a box for each orbital in any given principal energy level.

Question 13

Hund’s Rule

Answer 13

The rule stating that the lowest energy state for an atom has the maximum number of unpaired electrons allowed by the Pauli exclusion principle in a given energy sublevel.

Question 14

Atomic Radius

Answer 14

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Question 15

Ionization Energy

Answer 15

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Question 16

Electron Affinity

Answer 16

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Question 17

Chemical Bonds

Answer 17

The force that holds atoms together in the form of an ionic compound or molecule.

Question 18

Lattice Energy

Answer 18

The energy that is given off as an ionic crystal forms from the gaseous ions of its elements.

Question 19

Polar Covalent Bond

Answer 19

A bond in which electrons are unequally shared between two atoms.

Question 20

Metallic Bond

Answer 20

The force of attraction between positively charged metal atoms, and the pool of valence electrons that moves among them.

Question 21

Co-ordinate Covalent Bond

Answer 21

A covalent bond in which one atom contributes both electrons to the shared electron pair bond.

Question 22

Resonance Structures

Answer 22

Two or more Lewis Structures that show the same relative position of atoms but different positions of electron pairs.

Question 23

Expanded Valence Energy Level

Answer 23

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Question 24

Valence-Shell Electron-Pair Repulsion Theory

Answer 24

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Question 25

Dipole

Answer 25

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Question 26

Intramolecular Forces

Answer 26

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Question 27

Intermolecular Forces

Answer 27

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Question 28

Dipole-Dipole Forces

Answer 28

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Question 29

Ion-Dipole Force

Answer 29

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Question 30

Ion-Induced Dipole Force

Answer 30

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Question 31

Dipole-Induced Dipole Force

Answer 31

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Question 32

Hydrogen Bonding

Answer 32

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Question 33

Crystalline Solids

Answer 33

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Question 34

Amorphous Solids

Answer 34

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Question 35

Atomic Solids

Answer 35

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Question 36

Network Solids

Answer 36

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Question 37

Allotropes

Answer 37

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Question 38

Ionic Crystal

Answer 38

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Question 39

Dalton’s Model

Answer 39

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Question 40

Photons

Answer 40

A quantum of electromagnetic energy that has particle-like properties.