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Chemistry > Atomic structure oxidation number and and redox > Flashcards

Atomic structure oxidation number and and redox Flashcards

Atomic structure oxidation number and and redox

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1
Q

Recall the number of electrons inhabiting the first 4 shells.

A

1 - 2
2- 8
3- 18
4- 32

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2
Q

Define orbital.

A

A region around the nucleus that can hold up to 2 electrons with opposite spins.

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3
Q

What is the shape of an S orbital?

A

Sphere

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4
Q

What is the shape of a P orbital?

A

Dumb-bell

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5
Q

How many orbitals make up an S-subshell?

A

One orbital

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6
Q

How many orbitals make up a P-subshell?

A

Three orbitals at right angles to one another.

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7
Q

How many orbitals make up a D-subshell?

A

Five orbitals

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8
Q

How many electrons can fill up an S subshell?

A

2

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9
Q

How many electrons can fill up a P subshell?

A

6

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10
Q

How many electrons can fill up a D subshell?

A

10

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11
Q

Why is subshell 4s filled first?

A

The 3D subshell si at a higher energy level than the 4s sub-shell.

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12
Q

Write the order of subshells in the electron configuration.

A

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

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13
Q

Complete the sentence…
Electrons fill orbitals…

And why does this happen?

A

Fill orbitals with the same energy singly before pairing.

This happens to prevent any repulsion between paired electrons.

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14
Q

What do roman numerals show in a compound name?

A

Shows the oxidation state of the element without a sign.

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15
Q

Define oxidation in terms of electron transfer.

A

Oxidation is loss of electrons

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16
Q

Define reduction in terms of electron transfer.

A

Reduction is the gain of electrons

17
Q

Define oxidation in terms of oxidation number.

A

Increase in oxidation number

18
Q

Define reduction in terms of oxidation number.

A

Decrease in oxidation number.

19
Q

What do the oxidation numbers of an ionic compound sum up to?

A

The relative charge of the ionic charge

20
Q

What do the oxidation numbers of a compound sum up to?

A

0

21
Q

What is ionic bonding defined as?

A

The electrostatic attraction between positive and negative ions.

22
Q

How is a giant ionic lattice formed?

A

Each ion attracts oppositely charged ions in all directions.

23
Q

Give some properties of ionic compounds.

A 
High melting and boiling points. 
Solid at room temperature . 
Dissolve in polar solvents.
Does not conduct electricity when solid.
Can conduct electricity when molten or dissolved.
24
Q

Why do ionic compounds have high melting and boiling points?

A

High temperatures are needed to overcome the strong electrostatic attraction between the ions.

25
Q

Why are ionic compounds solid at room temperature?

A

At room temperature there is insufficient amount fo energy to overcome the string electrostatic forces of attraction between the oppositely charged ions.

26
Q

Why do ionic compounds dissolve in polar solvents?

A

Polar water molecules break down the lattice and surround each ion in solution.
The water molecules attract and surround the ions because water is a polar molecules and has charged ends.

27
Q

Why do ionic compounds only conduct electricity when molten or dissolved?

A

When solid the ions are in a fixed position and are not mobile which prevents charge ti be carried in the structure however when the compound is molten or dissolved the solid ionic lattice breaks down and the ions are now free to move as mobile charge carriers.

28
Q

What is a covalent bond?

A

It is the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

29
Q 
How many bonds can the following form?
Carbon
Nitrogen
Oxygen
Hydrogen
A

Carbon- 4
Nitrogen- 3
Oxygen-2
Hydrogen-1

30
Q

What is a dative covalent bond?

A

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

31
Q

What is the measurement of covalent bond strength ?

A

Average bond enthalpy.

Chemistry (5 decks)

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