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Semester 1 Chemistry 11 > Topic 1 - Definitions > Flashcards

Topic 1 - Definitions Flashcards

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1
Q

Atomic number

A

of protons

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2
Q

Atomic mass

A

of protons + # of neutrons

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3
Q

Periods

A

Horizontal rows on the periodic table, helps identify the amount of electrons in an atom’s valence shell.

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4
Q

Groups

A

Vertical columns on the periodic table

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5
Q

Ionic bonding

A

bond between a M+NM; donates electrons to the other atom in the bond

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6
Q

Covalent Bonding

A

Co - to share electrons (NM + NM) –> polar covalent + non-polar covalent
Bond where valence electrons are shared equally between atoms usually occurring between non-metals

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7
Q

Metallic bonding

A

Bond between 2 metals; governed by the metal activity series

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8
Q

Valency

A

Combining power of an element which is equal to the number of electrons added, removed or shared when it is bonded with other atoms

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9
Q

Atomic radius

A

Measures the size of an atom and is defined as the average distance from the centre of the nucleus to the boundary of the valence shell

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10
Q

Force of attraction

A

How much the outer electrons (-) are attracted to the nucleus –> easily lost

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11
Q

Electronegativity

A

The tendency of an atom to attract electrons during a chemical bond

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12
Q

Chemical property

A

characteristics or behaviour of a substance that may be observed when it undergoes a chemical reaction

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13
Q

Electron Configuration - Subshell notation

A

S shell - holds max of 2 electrons (left side of the periodic table: metals, including helium)
P shell - holds max of 6 electrons (right side of the periodic table: non-metals)
D shell - holds max of 10 electrons (centre of the periodic table: transition metals)

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14
Q

Polyatomic ions

A

Two or more atoms in a bond giving the compound an overall charge

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15
Q

Electron affinity

A

The change in energy (kJ/mole) of a neutral atom when an electron is added to the atom, forming an anion

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16
Q

VSEPR Theory

A

Valence Shell Electron Pair Repulsion Theory

  • the role of electron pairs in shaping the arrangement of atoms in molecules
  • the theory proposes that all electron pairs in atoms repel each other mutually
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17
Q

Predicting shapes of simple molecule:

A
  1. Identify the atom of highest covalence and have it in the centre
  2. Draw an electron-dot diagram
  3. Count the number of bonding + non-bonding pairs
  4. Identify arrangement of electron pairs
  5. Identify electron shape and draw
18
Q

Polarity

A

The distribution of electrical charge over the atoms joined by the bond

19
Q

Polar Covalent

A
  • Have a negative and positive pole
  • Happens when 2 non-metals are in a bond
  • One has a higher electronegativity than the other
  • This causes one atom to be slightly positive and the other slightly negative
  • All halogens are polar covalent (H2, F2, BR, Cl2, O2, I2, N2)
  • Polar covalent substances dissolve easier than non-polar covalent
20
Q

Non-Polar covalent

A
  • Between the same element
  • Happens when atoms are of equal electronegativity or due to the molecular shape
  • Both poles are the same charges (+ , +) or (- , -)
21
Q

Predicting if the covalent bond is Polar or Non-Polar

A
  1. Assign partial charges (S-, S+)
    • due to electronegativity
    • anything with a low electronegativity will usually be S+
  2. Assign an arrow to indicate area of low E.N and area of high E.N (low EN = + high EN = - )
22
Q

Solution

A

A homogenous mixture consisting of a solute dissolved into a solvent
- solute: substance that is being dissolved
- solvent: dissolving medium
When one substance dissolves into another, a solution is formed

23
Q

Water (H2O)

A

Known as the universal solvent as it can dissolve the most substances

24
Q

Ionic Compounds

A

Can conduct electricity when molten (liquid) or in aqueous solution (dissolved in water) because their ions are free to move from place to place

25
Q

Dissociation

A

A process where ionic substances break apart when dissolved in water

26
Q

Linear

A

Any molecular with only two atoms. Also, if same atom, non-polar halogens (diatomic), N2, O2, H2. If 2 atoms are different, they are polar

27
Q

What is #protons equal to?

A

Electrons

28
Q

Polyatomic Ions Tip: If it ends with ‘ate’ the polyatomic ion has…

A

More oxygen than ‘ite’

29
Q

Polyatomic Ions Tip: If it ends with ‘ide’ it has…

A

No oxygen

30
Q

What is physical change?

A

A change observed that does not alter the chemical identity of the molecule but changes state of matter. Solid –> Liquid –> Gas

31
Q

What are the physical properties of materials? (elements, compounds, mixtures)

A
  • Melting point
  • Boiling point
  • Electrical conductivity
  • Thermal conductivity
  • Mass
32
Q

What is melting point?

A
  • The temperature range which causes the material to change from solid to liquid
  • Chemistry concept: Heat energy causes the atoms to vibrate and in turn faster (kinetic energy)
  • Atoms vibrate away from each other causing the bond between the molecules to be less tightly packed
33
Q

What is boiling point?

A
  • The temperature range which causes the material to change from liquid to gas
  • Chemistry concept: Heat energy causes the atoms to vibrate and in turn faster (kinetic energy)
  • Atoms vibrate away from each other causing the bond between the molecules to be less tightly packed
  • It is the result of transferring higher heat energy compared to melting point
34
Q

What are the characteristics of metals?

A
  • Shiny
  • Mostly solid at room temperature, some exceptions are liquids
  • conducts electricity
  • Conducts heat
  • Ductile
  • Malleable
  • Not all metals react the same though
35
Q

What are some common reactions with metals?

A
  1. When metals react with oxygen, they produce a metal oxide.
    E.g. calcium + oxygen –> calcium oxide
  2. When metals react with water, they produce a metal hydroxide
    E.g. sodium + water –> sodium hydroxide
  3. When metals react with acids, they produce metal salt and hydrogen gas
    E.g. magnesium + hydrochloric acid –> magnesium chloride + hydrogen
    (THESE REACTIONS DO NOT OCCUR FOR EVERY METAL, IT DEPENDS ON THEIR REACTIVITY)
36
Q

Trigonal Planar

A
  • A molecular with three electron groups orients the three groups as far apart as possible.
  • They adopt the positions of an equilateral triangle - 120° apart and in a plane shape.
37
Q

Inter and Intra Molecular Bonds

A

Intermolecular bonds are the forces between the molecules

Intramolecular bonds are the forces within two atoms in a molecule

38
Q

Primary bonds or intramolecular forces

A

Strong attractive forces that joins atoms in a molecule

39
Q

Secondary interactions or intermolecular forces

A

Weak attraction forces that joins 2 elements, which includes London dispersion-forces, dipole-dipole interactions and hydrogen bonding

40
Q

London dispersion forces

A

Exists between all molecules. Their strength depends on the size and shape of the molecules.

  • weakest intermolecular force
  • temporary attractive force that occurs when the electrons in 2 adjacent atoms occupy positions that make the atoms form temporary dipoles
41
Q

Ionization energy

A

The amount of energy needed to remove an outer electron from an atom and make it into an ion

Semester 1 Chemistry 11 (4 decks)

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