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Chemistry (shubh) > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

Order the following: shells, subshells and orbital services

A

Shells made of subshells

Subshells made of orbitals

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2
Q

How many electrons per orbital

A

2 paired electrons

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3
Q

How many orbitals in s subshell

A

1

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4
Q

How many orbitals in p subshell

A

3

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5
Q

How many orbitals in d subshell

A

5

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6
Q

Subshells in shell 1

A

Only s

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7
Q

Subshells in shell 2

A

S and p

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8
Q

Subshells in shell 3

A

S,p and d

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9
Q

Subshells in shell 4

A

S,p,d and f

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10
Q

Number of electrons per shell number

A

2,8,18,32

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11
Q

What does this mean:

3P subscript 6

A

Shell number 3
Orbital p
6 electrons in those orbitals

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12
Q

Shape of s orbital?

S orbital shape of higher shells?

A

Sphere

Higher shells are larger in volume but same shape

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13
Q

Why do higher shell orbitals have higher volume

A

Higher shell electrons have more energy so on average they are further away from the nucleus

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14
Q

What do the orbitals actually represent?

What are the chances of finding an electron in the orbital?

A

The area around a nucleus where there is a high chance of finding an electron

but they move randomly and we have no idea of the electron’s direction or speed so theoretically they can be anywhere in the universe

95%

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15
Q

Shape of p orbital

A

Two lobes of same size which align with axes that they are named for. 3 orbitals in x y and z axis so perpendicular to each other. All three are equal energy

Dumbell shape

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16
Q

Shape of d orbital

A

4 lobes and one very strange shape all with equal energy

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17
Q

Why do two electrons in same orbital have opposite spin

A

Same charge so repel

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18
Q

What is an electron cloud

A

An orbital where an electron can potentially be found

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19
Q

How would you arrange 4 electrons in a p orbital

A

2 paired electron in first square

And 1 each in the other two squares

20
Q

How do you remember order of energy

A

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

Diagonally down

21
Q

Why does copper and chromium only have 1 electron in 4s orbital?

A

Stability because having full orbitals or half full sets of orbitals is more stable and favourable energetically

22
Q

1s2 2s2 2p6 3s2 3p6 4s2 3d2

This atom becomes an ion and loses 2 electron
What is its config or from which orbital is the electron lost

A

4s2 orbital loses both electrons because of first in first out rule

When filling 4s is lower in energy so filled first but once filled it becomes higher energy so it is lost before 3d

23
Q

3/4 rules of electron config in the orbitals

A

Fill electron with lowest energy level first

Only 2 electron in an orbital with opposite spins

Each orbital has 1 electron before 2nd is introduced or paired

24
Q

What is shorthand rule

Any example?

A

Using previous noble gas and then add in outer electron subshells as normal

Na = Ne in square brackets then 3s1

25
Q

What is ionic bonding

A

Electrostatic attraction between oppositely charged ions

26
Q

Why is the ionic bonding structure a giant lattice

A

Each ion attracts oppositely charged ions in all directions

27
Q

Finish sentence

The greater the … the stronger the electrostatic attraction between them

A

Charge

28
Q

What is ionic bonding bp/mp like and why

A

Mp/bp is high cos ionic is strong bond so lots of energy needed to overcome this bond

29
Q

What do ionic substances dissolve in or do they not

Do all ionic compounds dissolve

A

Polar solvents like water

Large charged compounds don’t dissolve as the bond is too strong

30
Q

Which atom in h20 water has a positive dipole

A

H

31
Q

Why does oxygen have a negative dipole in water

A

It has 2 lone pairs of electrons so that area has slight negative charge

32
Q

How does water break down ionic lattice

A

H20 molecules pull ions apart by surrounding each ion which eventually breaks down the lattice

33
Q

Why doesnt ionic compound conduct at solid

A

Ions are in foxed position and only vibrate on the spot

34
Q

Why do ionic compounds conduct in aqueous or molten

A

Ionic lattice breaks down

Ions are free to move as mobile charge carriers

35
Q

What is covalent bond

A

Strong electrostatic attraction between a shared pair of electrons and nuclei of the bonded atoms

36
Q

Why do simple molecular covalent have weak intermolecular forces

A

The attraction of covalent bonding is only localised to the nuclei of the multiple atoms

37
Q

What is intermolecular force

What is intramolecular force

A

Weak forces between different molecules

The actual covalent bond between the atoms

38
Q

Which is stronger ionic or giant covalent

A

Giant covalent

39
Q

What is a lone pair of electrons

A

Paired electrons that aren’t shared with another atom

40
Q

What are simple molecular soluble in

And how/why

A

Non polar solvents like benzene

Van der waals forces form between solvent and molecule which weakens the lattice

41
Q

What are the 3 giant covalent structures for a level

A

Graphite
Diamond
Silica or silicon dioxide

42
Q

What are giant covalent soluble in

Why

A

Neither polar nor non polar as the bonds are too strong

43
Q

Graphite properties and reason

A

Slippery as the layers have weak intermolecular forces between them

Conductive as there are extra electrons that form clouds of free electrons between the layers

44
Q

What is a dative bond

A

Only the bonding atom supplies both electrons as the shared pair as the shared pair was originally a lone pair of electrons

45
Q

What is average bond enthalpy

A

Measurement of covalent bond strength

Larger the value the stronger it is

46
Q

Complete sentence

Covalent bonds have paired electrons that have same electron config as nearest noble gas which obeys the …… rule

A

Octet

47
Q

Why is it not always possible to follow octet rule

2 points

A

May not have enough electrons to reach full octet

Have more electrons available as it can access the d orbitals so octet expands.

Chemistry (shubh) (9 decks)

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