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A LEVEL CHEMISTRY > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

How many electrons can fill the first energy level?

A

Two electrons fill the first energy level

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2
Q

How many electrons can fill the second energy level?

A

Eight electrons can fill the second energy level

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3
Q

How many electrons can fill the third energy level?

A

Eighteen electrons can fill the third energy level

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4
Q

How many electrons can fill the fourth energy level?

A

Thirty two electrons can fill the fourth energy level

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5
Q

What is the general formula for number of electrons

A

The general formula for number of electrons is 2n^2

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6
Q

How many sub shells are there and what are their names?

A

There are four sub shells called: s,p, d and f.

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7
Q

Definition of an atomic orbital

A

And orbital is a region around the nucleus that can hold up to 2 electrons with opposite spins

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8
Q

What shape is an S orbital

A

And S orbital is spherical

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9
Q

What shape is a p orbital

A

Appeal battle is dumb bell shaped

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10
Q

How many orbitals are there in an S subshell and how many electrons can an s sub shell hold ?

A

An s subshell has one orbital this can hold 2 electrons

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11
Q

How many orbitals does a p sub shell have and how many electrons can a p subshell hold?

A

A p sub shell has three orbitals thus can hold six electrons

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12
Q

How many orbitals does a D subshell have and how many electrons can it hold?

A

A D subshell has five orbitals thus can hold 10 electrons

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13
Q

When is filling orbitals in the same energy level should you occupy singly or pair first?

A

For all the tools in the same energy level occupy singly before pairing

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14
Q

How do you write a shorthand electron configuration?

A

Write a shorthand electron configuration by putting the symbol of the previous noble gas in square brackets then the outer electron shells next to it

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15
Q

Which subshell is the exception to the rule?

A

The 4S subshell is an exception because it is filled before the 3-D subshell as it is at low energy

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16
Q

Definition of isoelectronic

A

I saw electronic – two ions that possess the same electronic configuration

17
Q

Definition of ionic bonding

A

Ionic bonding is the electrostatic attraction between positive and negative ions

18
Q

What do ionic compounds look like?

A

And it compounds from giant ionic lattices as charged ions attract oppositely charged ions in all directions

19
Q

Why are ionic compounds solid at room temperature?

A

Ionic compounds are solid at room temperature as there is insufficient energy to overcome the electrostatic forces between oppositely charged ions in the lattice

20
Q

Why do ionic compounds have high melting and boiling points

A

Ionic compounds have high melting points and boiling points because lots of energy is needed to overcome the electrostatic forces of attraction between oppositely charged ions in all directions. Ionic compounds with greater charges have higher melting and boiling points

21
Q

Are ionic compounds soluble?

A

Ionic compounds are soluble in polar solvents such as water as the polar molecules are Attracted to the irons and pull them away from the lattice causing them to dissolve

22
Q

Do ionic compounds conduct electricity?

A

Ionic compounds conduct electricity when molten or dissolved as the ions are free to move as mobile charge carriers

23
Q

Definition of a covalent bond

A

A covalent bond is strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

24
Q

Covalent bonding which elements are exceptions to the octet rule?

A

Boron, Phosphorus, sulphur and chlorine are exceptions to the octet rule

25
Q

What covalent molecule does boron form that is an exception to the octet rule?

A

Boron forms BF3

26
Q

What covalent molecules does Phosphorus form that is an exception to the octet rule?

A

PF3 and PF5

27
Q

What covalent molecules does Sulfur form that is an exception to the octet rule?

A

SF2, SF4 and SF6

28
Q

What covalent molecules does Chlorine form that is an exception to the octet rule?

A

ClF, ClF3, ClF5 and ClF7

29
Q

What is a dative covalent bond?

A

A dative covalent bond is where both electrons are donated from one atom

30
Q

What is average bond enthalpy

A

Average bond enthalpy is a measurement of covalent bond strength. The larger the bond enthalpy the stronger the bond

A LEVEL CHEMISTRY (21 decks)

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