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Chemistry 12 > Unit 1 - Structure and Properties of Matter > Flashcards

Unit 1 - Structure and Properties of Matter Flashcards

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1
Q

Electromagnetic Radiation

A

a form of energy

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2
Q

Electromagnetic Spectrum

A

the range of wavelengths or frequencies over which electromagnetic radiation extends (radio -> gamma). The most energetic waves has the highest frequency

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3
Q

Wavelength (lambda)

A

the distance between two consecutive peaks or troughs, length go one cycle

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4
Q

Frequency (nu)

A

waves(cycles)/sec , how often something occurs

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5
Q

Planck’s Quantum Theory

A

atoms and molecules could emit or absorb energy only in discrete quantities

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6
Q

Quantum (the energy of a photon of light)

A

the smallest quantity of energy that can be emitted or absorbed in the form of electromagnetic radiation. Plural is quanta

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7
Q

Photons

A

particles of light

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8
Q

Heisenberg Uncertainty Principle

A

You can not know the position and momentum of an electron/particle at the same moment in time.

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9
Q

Orbital

A

wave function of an atom

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10
Q

Principal Quantum Number

A

energy level and size of orbital (n)

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11
Q

Angular Momentum Quantum Number

A
  • shape/type of orbital - which sub shell the electron is found in (l = n-1) The higher the value of l, the greater is the energy of the subshell within an energy level.
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12
Q

Magnetic Quantum Number

A

spacial orientation/ where to find electron in (ml=2l+1)

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13
Q

Spin Quantum Number

A

orientation of spin of axis (ms) - +ve spin goes in first

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14
Q

Pauli Exclusion Principle

A

no two electrons in the same atom can have identical values for all four of their quantum numbers

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15
Q

Aufbau Principle

A

The aufbau principle states that in the ground state of an atom or ion, electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels (e.g., 1s before 2s). In this way, the electrons of an atom or ion form the most stable electron configuration possible.

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16
Q

Orbital diagram

A

square diagrams showing the electrons and spin in orbitals of equal energy

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17
Q

Electron Configuration short cut

A

use name of last noble gas, then follow it with the orbitals

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18
Q

Hund’s Rule

A

the most stable electron arrangement for an atom is the one with the highest number of unpaired electrons with parallel spins (spinning optimally at this point)

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19
Q

Excited State

A

when an electron absorbs energy, it moves to a higher shell or subshell

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20
Q

Ground State

A

all of the electrons are in as low an energy level as it is possible for them to be

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21
Q

Exceptions to Configuration

A

The electronic configurations of several elements such as Cr, Cu, Ag, Pt and Au do not follow the general rule. In each one of these, the atom is more stable when the highest occupied s subshell has one electron instead of two, and the highest occupied d subshell has one more electron than it should have.

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22
Q

Atomic radius

A

increases down period, decreases down group (because of protons, ENC, and shielding)

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23
Q

Ionization Energy

A

the minimum energy required for removing an electron from the highest occupied subshell of an atom or an ion at its gaseous, ground state (decreases down and increases across because of protons, ENC, and shielding)

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24
Q

Electronegativity

A

the ability of an atom to attract electrons in a bond

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25
Q

Covalent Bond

A

chemical bond that involves the sharing of electron pairs between atoms

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26
Q

Nonpolar covalent bond

A

bonding electrons shared equally between 2 atoms, no charges on atoms

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27
Q

Polar covalent bond

A

bonding electrons shared unequally between 2 atoms, partial charges on atoms

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28
Q

Ionic bond

A

complete transfer of one or more valence electrons

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29
Q

Zero Energy State

A

energy that electron has at ground state

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30
Q

Infinite Separation Point

A

at the point where there is no loner an electrical force of attraction

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31
Q

Internuclear Distance

A

distance between the two atoms/ions (if your atoms have more protons the distance will be greater)

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32
Q

Bond Length

A

distance between the nuclei at the most stable state, lowest potential energy

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33
Q

Lattice Energy

A

Energy required for an ionic bond

34
Q

Sublimation

A

change of state from solid to gas

35
Q

Ep in energy levels

A

As energy levels increase, distance from nucleus increases. This results in decreased stability and force of attraction, with an increase in Ep.

36
Q

Electron affinity

A
  • Energy change associated with adding electron in ground state - wants full shell and more protons, weakens ENC - exothermic reaction - the more it wants it the more -ve, favourable - 1/2 full have low affinities
37
Q

What is nf value at infinite separation?

A

It would be 0 because 1/infinity = 0

38
Q

Coulomb’s Law

A

the larger the charges on top, the more stable it is because the nuclei are closer together with greater force of attraction and smaller the distance. The smaller the distance means more energy required.

39
Q

Endothermic

A

absorb energy

40
Q

Exothermic

A

release energy

41
Q

Lewis structure

A
  • Shows arrangement of valence electrons
  • For ionic compound electrons are transferred
  • For molecular compounds electrons are shared to become electrically stable
42
Q

Lone pairs

A

unshared electrons

43
Q

Bonding pairs

A

Shared electrons (i.e sigma and pi)

44
Q

Elements that require octet rule

A

Carbon, nitrogen, oxygen and fluorine

45
Q

Coordinate covalent bond

A

When completing an octet, bond is contributed by one of the two atoms

46
Q

Free radical

A

Highly reactive molecule containing unpaired electrons

47
Q

VSEPR

A

Valence shell electron pair repulsion

  • predict geometry using Lewis structure
  • repulsion of electron pairs around central atom determine shape
48
Q

Loan pairs impact shape by…

A
  • Cause more repulsion against electrons
  • Change bond angle
49
Q

Sigma bond

A

Single bond, head-on head overlap with electron density between nuclei

50
Q

Pi bond

A

head on head sideways overlap, above and below bond axis, do not repel each other because attracted by same nuclei

51
Q

Structural pairs

A

Determine geometry, Sigma and lone pairs

52
Q

2 structural pairs

A

Hypridization- sp

53
Q

3 structural pairs

A

Hybridization- sp2

54
Q

4 structural pairs

A

Hypridization- sp3

55
Q

5 structural pairs

A

Hypridization- sp3d

56
Q

6 structural pairs

A

Hypridization- sp3d2

57
Q

Hybridization

A
  • When electron configuration does not support molecular geometry electrons get promoted to orbitals of same n value
  • Different orbital shapes merged together in order to have identical size and shape
  • Only structural pairs determine hybrid
  • Hybrid orbitals are half-full
58
Q

Intermolecular force

A

Electrical forces of interaction between molecules, weaker

  • LDF, dipole-dipole, hydrogen bonding
59
Q

Intramolecular force

A
  • attraction that holds together molecule
60
Q

London dispersion forces

A
  • Temporary dipole/polarity and induced dipoles
  • Larger or electron cloud = higher boiling point ->Due to an increase of electrons where there are more temporary dipoles in the molecule and greater dipole distance
  • If able to stack closer because of shape, higher boiling point
61
Q

Dipole dipole interactions

A
  • Molecules with pernament dipoles, considerable electronegativity
  • Have boiling points higher than molecules with LDF
  • Boiling point between polar and nonpolar depend on size and number of electrons
62
Q

Hydrogen bonding

A
  • Strongest dipole dipole interaction (N, O, F)
  • Close up approach of dipoles allowed by small hydrogen
  • Results in even greater boiling point
63
Q

Dipole induced dipole

A

Interaction between polar and nonpolar molecule

64
Q

Ion - dipole interaction

A

Interaction between polar molecule and ions

65
Q

Crystalline solid

A

Atoms, ions or molecules make up underlying structure with regular repeating patterns, breaks smoothly and in cleavage

66
Q

Amorphous solid

A

Do not have much order, more chaotic and rigid

67
Q

Four types of crystalline solids

A
  1. Ionic solids
  2. Molecular solid
  3. Covalent network solid
  4. Metallic solid
68
Q

Type of Solid: Ionic Solid

Melting Point:

Hardness:

Conductivity:

A

Type of Solid: Ionic Solid (must have charge)

  • made up of positive and negative ion held together by electrostatic forces

Melting Point: high to very high

Hardness: hard and brittle

Conductivity: nonconducting solid and conducting liquid

69
Q

Type of Solid: Molecular Solid

Melting Point:

Hardness:

Conductivity:

A

Type of Solid: molecular solid

  • made up of atoms or molecules held together by intermolecular forces

Melting Point: low

Hardness: soft to brittle

Conductivity: non-conducting

70
Q

Type of Solid: Covalent network solids

Melting Point:

Hardness:

Conductivity:

A

Type of Solid: Covalent network solids (mostly names)

  • made up of atoms connected through a network of covalent bonds, no distinction between intra and intermolecular forces, graphite and diamond

Melting Point: very high

Hardness: very hard

Conductivity: usually non-conducting (graphite is an exception)

71
Q

Type of Solid: Metallic Solid

Melting Point:

Hardness:

Conductivity:

A

Type of Solid: Metallic Solid

  • consists of positive cores of atoms held together by sea of electrons

Melting Point: varies

Hardness: variable hardness and malleable

Conductivity: conducitng

72
Q

Melting/fusion

A

change of state from solid to liquid

73
Q

Freezing

A

change of state from liquid to solid

74
Q

Vapourization

A

change of state from liquid to gas

75
Q

Condensation/ liquefaction

A

change of state from gas to liquid

76
Q

Condensation/ deposition

A

change of state from gas to solid

77
Q

Alloys

A

a metal made by combining two or more metallic elements

Interstitial alloy: compound that is formed when an atom of sufficiently small radius sits in an interstitial “hole”

Substitutional: atoms of the solute metal take the place of some atoms of a metal of similar atomic radius

78
Q

Vapour pressure

A
  • In a liquid is the pressure exerted by the vapor and dynamic equilibrium with the liquid at a constant temperature
  • Larger molecules have lower vapor pressure as a result of a lower vaporization rate
  • Vapor pressure and atmospheric pressure are inversely proportional
79
Q

Dynamic equilibrium

A

When vaporization rate = condensation rate

80
Q

Boiling point

A
  • out of certain temperature vaporization occurs throughout the liquid in an open container
  • when vapor pressure equals atmospheric pressure
81
Q
A
82
Q
A

Chemistry 12 (1 decks)

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