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IB Chemistry > Unit 1 The periodic table > Flashcards

Unit 1 The periodic table Flashcards

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1
Q

Define relative/natural abundance

A

Is a consistent ratio found in nature for given elements.

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2
Q

What is atomic mass of an element?

A

Is the weighted average of the mass of its isotopes.

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3
Q

Define weighted average

A

means some values have greater impact of the average than others.

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4
Q

What are some important points when calculating relative abundance?

A
  • the larger isotope number is “x”

- the first step to isolating “x” is to multiply both sides by 100

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5
Q

What are the two rules that need to be followed for adding electrons to the orbital box diagrams?

A

1) Pauli Exlusion Principle

2) Hund’s Rule

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6
Q

Describe the two rules for the orbital box diagram

A

Pauli Exclusion Principle:
- The maximum number of electrons in each orbital is two. If two electrons are in one orbital, they must have opposite spins.
Hund’s rule:
- When adding electrons to a sublevel with more than one orbital, the electron spins must be all the same until each orbital has one electron.

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7
Q

What is the Aufbau principle?

A

Electrons fill sublevels starting with the lowest energy level up to highest energy.

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8
Q

State the limitations of the Bohr Model

A

Assumes or suggests:

  • electrons orbit the nucleus/is predictable
  • shape of orbits/shells are all spherical
  • an incorrect scale of an atom
  • energy of electrons in a level are all the same
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9
Q

What are the exceptions to the full electron configuration?

A
  • Nearly full “d” sublevels will take an electron from the closest “s” sublevel to be full
  • Nearly half full “d” sublevels will take an electron from the closest “s” sublevel to be half full
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10
Q

What is the electromagnetic spectrum order in increasing energy?

A

Radiowaves, Microwaves, infrared, visible, untraviolet, x-rays, gamma rays

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11
Q

How are the elements of the periodic table arranged?

A

By increasing atomic number

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12
Q

What is the significance of the periodic groups?

A

The elements in the groups have similar chemical properties.

- same number of valence electrons

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13
Q

What is the name of group 1?

A

Alkali metals

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14
Q

What is the name of group 2?

A

Alkaline earth metals

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15
Q

What is the name of groups between group 2 and 3?

A

Transition metals

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16
Q

What is the name of group 6?

A

Chalcogens

17
Q

What is the name of group 7?

A

Halogens

18
Q

What is the name of group 0 (or 8)?

A

Nobel gasses or inert gasses

19
Q

What is the name of the two lower rows?

A

Rare earth elements

20
Q

What are the horizontal rows called and what is their significance?

A

Called periods

- the number of the period equals the number of energy levels in the ground state

21
Q

What is Atomic Radius?

A

The distance from the nucleus to the outermost electron.

22
Q

How do you find atomic radius?

A

Half the distance nuclei of two bonded atoms of the same element (ex. diatomic molecules)
- is estimated for non-identical atoms

23
Q

What is Ionic Radius?

A

Defined as the distance from the nucleus to the outermost electron of an ion

24
Q

Describe on general terms the ionic radius of the ions

A
  • Cations loose electrons and are smaller than their respective atom, occurs for metals.
  • Anions have gained electrons and are larger than their respective atom, occurs for non-metals.
25
Q

Define First Ionization Energy

A

The energy needed to remove one electron from an atom in its gaseous state.

26
Q

Define electronegativity

A

Is a relative measure (having no units) of the attraction an atom has for a pair of electrons that are shared with another atom.

27
Q

Define electron affinity

A

The energy released when one electron is added to an atom in its gaseous state. (only applies to non-metals)

28
Q

What is the periodic trend for atomic radius?

A

Atomic Radius:

  • increases down the group because an extra shell is added
  • decreases across the period because there are more protons
29
Q

What is the periodic trend for ionic radius?

A

Ionic Radius:

  • increases down the group because an extra shell is added
  • decreases across the period because there are more protons
30
Q

What is the period trend for ionization energy?

A

Ionization Energy:

  • decreases down the group because an extra shell is added
  • generally increases across the period because there are more protons
31
Q

What is the periodic trend for electronegativity?

A

Electronegativity:

  • decreases down the group because an extra shell is added
  • increases across the period because there are more protons
32
Q

What is the period trend for electron affinity?

A

Electron Affinity:

  • generally decreases down the group because an extra shell is added
  • generally increases across the period because there are more protons
33
Q

What is the general trend for melting point?

A

Melting Point:

  • For Alkali metals the melting point decreases down the group
  • For Halogens melting point increase down the group
  • Across periods 2 and 3 melting point increases from group 1 to 4 and generally decreases from group 4 to 0
34
Q

What is the first type of reaction?

A

2(Alkali metal) + 2H20 -> 2(Alkali metal ion) + 2OH^- + H2

35
Q

What is the second type of reaction?

A

2(Alkali metal) + Cl2 or Br2 -> 2(Alkali metal)Cl or Br

36
Q

What is the third type of reaction?

A

(greater electronegativity halogen)2 + 2(lower electronegativity halide ion) -> 2(greater electrnegativity halide ion) + (lower electronegativity halogen)2

2(greater electronegativity halide ion) + (lower electronegativity halogen)2 -> No reaction

37
Q

What is the fourth type of reaction?

A

Metal oxide + Water -> metal hydroxides

38
Q

What is the fifth type of reaction?

A

non-metal oxide + water -> acidic oxide

IB Chemistry (8 decks)

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