Electron Configuration and Structure Flashcards Preview

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Flashcards in Electron Configuration and Structure Deck (45)
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1
Q

Define electron configuration?

A

The arrangement of electrons in an atom

2
Q

How are electron arranged in an atom?

A

In energy levels/ shells numbered linearly, with number 1 being closest to the nucleus.

3
Q

What are the first 10 energy levels in electron configuration?

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 4d, 4f

4
Q

What are subshells made up of?

A

Subshells are made up of orbitals - a region the nucleus that can hold up to 2 electrons with opposite spin.

5
Q

What do orbitals represent?

A

They represent the mathematical probabilities of finding an electron at any point within certain spatial distributions around the nucleus.

6
Q

What is the Aufbau principle?

A

Electrons fill up the lowest energy subshells first

7
Q

What is the Pauli exclusion principle?

A

Electrons fill up orbitals singly before pairing up

8
Q

What is the Hund’s rule?

A

Each orbital holds 2 electrons with opposite or ‘paired spins’

9
Q

What is the exception in the pattern that orbitals fill up in?

A

The 4s- subshell is filled before the 3d- subshell.

10
Q

When is a cation formed?

A

Formed when electrons are lost

11
Q

When is an anion formed?

A

Formed when electrons are gained

12
Q

What rule do Hydrogen and Helium follow?

A

The duet rule

13
Q

What are the four types of chemical bonds?

A
  1. Ionic
  2. Covalent
  3. Metallic
  4. Dative covalent
14
Q

What is an ionic bond?

A

An electrostatic attraction between oppositely charged ions. Ionic bonds act in all different directions so each ions will be surrounded on all sides by ions of the opposite charge.

15
Q

When is an ionic bond formed?

A

Results from electron transfer from a metal atom to a non-metal atom.

16
Q

What is a covalent bond?

A

An electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms. Sigma bonds are formed by the overlap of an s and p orbital or 2 p-orbitals meeting end to end.

Covalent bonds are directional unlike ionic bonds

17
Q

When is a covalent bond formed?

A

Occurs between non-metal atoms and each atom provides an electron for the bonded pair

18
Q

What is a dative covalent bond and when is it formed?

A

In dative covalent bonds, one atom provides both electrons for the bonded pair

19
Q

What is metallic bonding and how is it formed?

A

Electrostatic attraction between a lattice of metal cations and delocalised electrons.

20
Q

What do dot and cross diagrams show?

A

The bonding of the outer shell electrons

21
Q

What is a lone pair?

A

A pair of non-bonded electrons

22
Q

How many covalent bonds can Hydrogen make?

A

1

23
Q

How many covalent bonds can Oxygen make?

A

2

24
Q

How many covalent bonds can Nitrogen make?

A

3

25
Q

How many covalent bonds can Carbon make?

A

4

26
Q

What is the substance if there is no bonding?

A

A monoatomic gas

27
Q

What are the two main structures of bonding?

A
  1. Giant lattice structures

2. Simple covalent structures

28
Q

What is a giant lattice structure?

A

Have a regular 3-D arrangement of atoms which extends throughout the compound

29
Q

What is a simple covalent structure?

A

Consists of many small molecules held together by weak intermolecular forces.

30
Q

When do giant lattice structures occur?

A

In ionic compounds

31
Q

What is the melting point of giant lattice structure like? why?

A

High melting point because lots of energy is required to break the strong ionic bonds in the lattice.

32
Q

Are giant lattice structures soluble in water?

A

Often

33
Q

Do giant lattice structure conduct electricity? Why?

A

Yes when molten or in solution because ions become free to move as mobile charge carriers.

34
Q

When do simple covalent molecular structures occur?

A

Occurs in small covalent molecules

35
Q

What is the melting point of simple covalent molecular structures like? why?

A

Low melting point as little energy is required to break weak intermolecular forces

36
Q

Are simple covalent molecular structures soluble in water?

A

Often insoluble in water

37
Q

Do simple covalent molecular structures conduct electricity? Why?

A

Do not conduct electricity as lack mobile ions or electrons to act as charge carriers.

38
Q

When do Giant covalent lattice structures occur?

A

Found in diamond, graphite, silica etc

They have a lattice of strong covalent bonds throughout the compound

39
Q

What is the melting point of Giant covalent lattice structures like? why?

A

Very high melting point because a large amount of energy is required to overcome the covalent bonds

40
Q

Are Giant covalent lattice structures soluble in water?

A

Usually insoluble

41
Q

Do Giant covalent lattice structures conduct electricity? Why?

A

Do not conduct electricity except graphite

42
Q

When do Giant metallic lattice structures occur?

A

Strong electrostatic attraction between metal cations and delocalised electrons

43
Q

What is the melting point of Giant metallic lattice structures like? why?

A

High melting point because of strong intermolecular forces

44
Q

Are Giant metallic lattice structures soluble in water?

A

Usually insoluble in water

45
Q

Do Giant metallic lattice structures conduct electricity? Why?

A

Conduct electricity when molten or solid because delocalised electrons are free to move as mobile charge carriers.