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Chemistry Module 2 > 5: Electron Configuration, Ionic, Covalent, Metallic Bonding > Flashcards

5: Electron Configuration, Ionic, Covalent, Metallic Bonding Flashcards

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1
Q

What is the principal quantum number?

A

The shell number.

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2
Q

Do shells have increasing or decreasing amounts of energy?

A

Increasing.

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3
Q

What is an alternate name for electron shells?

A

Energy levels

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4
Q

What formula is useed to calculate how many electrons can be in a shell?

A

2n^2, where n = shell number.

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5
Q

What can shells be broken down further into?

A

Subshells

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6
Q

How many different types of subshells are there?

A

4

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7
Q

How many electrons can an S subshell hold?

A

2

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8
Q

List the different types of subshells.

A

S, P, D, F

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9
Q

How many electrons can a P subshell hold?

A

6

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10
Q

How many electrons can a D subshell hold?

A

10

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11
Q

How many electrons can an F subshell hold?

A

14

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12
Q

What different subshells can be found on the first energy level?

A

S

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13
Q

What different subshells can be found on the second energy level?

A

S, P

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14
Q

What different subshells can be found on the third energy level?

A

S, P, D

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15
Q

What different subshells can be found on the fourth energy level?

A

S, P, D, F

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16
Q

What is each subshell made up of?

A

Orbitals

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17
Q

How many electrons can an orbital hold?

A

Up to 2, with opposite spin

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18
Q

How many orbitals can be found in an F subshell?

A

7

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19
Q

How many orbitals can be found in an D subshell?

A

5

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20
Q

How many orbitals can be found in an S subshell?

A

1

20
Q

How many orbitals can be found in an P subshell?

A

3

21
Q

What is the shape of the P orbital?

A

A dumbell figure of 8

22
Q

What is the shape of the S orbital?

A

A sphere

23
Q

Is it possible to, within a subshell, have 2 full orbitals and one empty orbital?

A

No, one electron occupies each orbital before pairing starts. This prevents any repulsion between paired electrons.

24
Q

What does the electron configuration of atoms show?

A

How subshells are occupied by electrons.

25
Q

What are the exceptions to the rule of electron configurations?

A

Copper, silver, gold, palladium, chromium, etc.

26
Q

How does the electron configuration confirm the period that an element is in (on the periodic table)?

A

Because the highest shell number will be the same as the period

27
Q

How does a difference in charge between ions increase the melting point of a compound?

A

The higher the difference in charge, the stronger the electrostatic attraction between oppositely charged ions. Therefore, the stronger the ionic bond will be, and the more energy it will require to break.

28
Q

What is an alternative name for a Dative Covalent Bond?

A

Co-ordinate bond.

29
Q

State 3 key giant covalent structures.

A

Diamond, Silicon Dioxide, Graphite.

30
Q

What do ions have the same structure as?

A

A noble gas.

31
Q

What is an ionic bond?

A

The electrostatic attraction between positive and negative ions to create an uncharged compound.

32
Q

A giant ionic lattice structure being formed is a result of what?

A

Ions attracting oppositely charged ions in all directions.

33
Q

What is a key structural feature of all ionic compounds?

A

A giant lattice

34
Q

Why do most ionic compounds have high melting and boiling points?

A

Because of the strong electrostatic forces of attractions between the oppositely charged ions that require a large amount of energy to overcome.

35
Q

Why do many ionic compounds dissolve in polar solvents?

A

-Polar molecules break down the lattice and surround each ion in solution
-In a compound made of ions with large charges, the ionic attraction may be too strong for water to be able to break down the lattice structure.

36
Q

Why won’t an ionic compound conduct electricity when solid?

A

The ions are in a fixed position in the giant ionic lattice, and there are no mobile charge carriers

37
Q

Why will an ionic compound conduct electricity when liquid or dissolved in water?

A

The solid ionic lattice breaks down, and the ions are now free to move as mobile charge carriers

38
Q

What is a covalent bond?

A

-Electrostatic attraction between a shared pair of electrons and the two nuclei.
-The overlap of atomic orbitals, each one containing one electron, to give a shared pair of electrons.

39
Q

What does covalent bonding occur between?

A

Non-metallic elements, compounds of non-metallic elements and polyatomic ions.

40
Q

Describe the attractions of covalent bonds.

A

They are LOCALISED attractions, meaning the attraction is only between the shared electrons and nuclei of the two bonded atoms

41
Q

What are the exceptions to the Octet rule?

A

-Boron (can hold 6 electrons in outer shell)
-Phosphorus (10 electrons)
-Sulfur (12 electrons)
-Halogens (14 electrons)

42
Q

What is a dative covalent bond?

A

A covalent bond where the shared pair of electrons has been supplied by one of the atoms only.

43
Q

Why can’t covalent compounds conduct electricity?

A

Because they have no overall charge, and no delocalised electrons.

44
Q

Describe a simple covalent structure.

A

-Isolated moelcules with weak forces between molecules
-Strong bonds between atoms, electrons are shared
-Low melting points, gases and liquids at room temp
-Doesn’t conduct electricity.

45
Q

Describe a giant covalent structure.

A

-Repeating 3D structure with strong bonds between atoms
-Electrons are shared
-High melting point, always solid at room temp
-Most don’t conduct electricity (except graphite)

46
Q

Describe the structure of metallic bonding.

A

-Positive ions surrounding by a “sea” of delocalised electrons
-Strong attraction between ions and delocalised electrions
-High melting points, almost all are solids at room temp
-Conduct electricity and heat
-Malleable

47
Q

Describe a giant ionic structure

A

-Regular 3D arrangement of positive and negative ions
-Strong electrostatic attraction between positive and negative ions
-High melting points, alwaus solid at room temp,
-Regular crystal arragnement
-Conduct electricity when molten or in solution.

Chemistry Module 2 (7 decks)

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