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Chemistry > Electrons, Bonding And Structure > Flashcards

Electrons, Bonding And Structure Flashcards

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1
Q

What are the blocks in the periodic table called?

A

S, d, p, f

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2
Q

How can you tell a covalent bond is present?

A

Hydrolysed by water

Liquid at rt

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3
Q

How are electrons arranged in an atom?

A

Around nucleus in shell.

Shell/sub shell/orbital

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4
Q

What happens to the energy of shells around the nucleus?

A

Further away= higher energy

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5
Q

What is a principle quantum number and what is the notation?

A

(n)

Measure of energy of shells

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6
Q

What is an orbital?

A

Region around nucleus that can hold up to 2 electrons

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7
Q

What is a sub shell?

A

Orbitals of same shape grouped together

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8
Q

What is a shell/energy level?

A

Different sub shells grouped together

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9
Q

Describe the s subshell

A

Spherical shape

One orbital

2 electrons max

Starts in first subshell

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10
Q

Describe p subshell

A

Dumbbell shape

3 orbitals (90 degrees to each other)

6 electrons max

Starts in second subshell

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11
Q

Describe d subshell

A

Five orbital

10 electrons max

Starts in third subshell

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12
Q

Describe f subshell

A

7 orbital

14 electrons max

Starts in fourth subshell

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13
Q

What is spin pairing and what is it represented by?

A

When two electrons are the same orbital (spin in opposite directions)

Shown by arrows

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14
Q

What are the electron configuration rules?

A

Lowest available energy level filled first (aufbau principle)

One orbital has max of 2 electrons with opposite spins

Electrons stay impaired for as long as possible in each subshell (Hunds rule)

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15
Q

What is Aufbau’s principle?

A

Lowest available energy level is occupied first

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16
Q

What is Hund’s rule?

A

Electrons stay impaired for as long as possible in each subshell

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17
Q

What parts of the periodic table occupy s,d,p and f blocks?

A

S= left

D= middle

P=right

F= bottom

18
Q

What do the s/d/p/f blocks in the periodic table signify?

A

Signify the last subshell with an electron in

19
Q

How does chromiums electron configuration end?

+why

A

3d5 4s1

Electron promotes from 4s2 to 3d4 to make 3D half full

20
Q

How does coppers electron configuration end?

+why?

A

3d10 4s1

Electron promotes from 4s2 to 3d9 to fill 3D

21
Q

Why is 4s filled and empties before 3d?

A

When empty 4s has lower energy than 3d.

When full 4s has a higher energy level than 3d

22
Q

What is an ionic bond?

A

The electrostatic force of attraction between positive and negative ions

23
Q

What are positive ions also know as?

A

Cations

24
Q

What are negative ions also know as?

A

Anions

25
Q

What is the structure of an ironically bonded compound ?

A

Giant ionic lattice

Giant=continually repeating units

Lattice =ions packed alternatingly

26
Q

Explain the melting and boiling points of ionic compounds

A

High

Strong forces of attraction between ions = lots of energy to overcome

27
Q

Explain the solubility of ionic compounds

A

Soluble in polar solvents = poles attract ions

insoluble in non-polar solvents (hydrocarbons)

28
Q

Explain the conductivity of ionic compounds

A

Good conductor of heat and electricity when molten or dissolved = ions free to move and carry charge

Poor conductor when solid = ions in fixed lattice position so cant move

29
Q

Explain the behaviour of ionic compounds when hammered

A

Brittle and easily cleaved

Layers distort when hammered, like charges align and repel.

30
Q

Define covalent bonding

A

The electrostatic force of attraction between a shared pair of electrons and the nuclei of two bonded atoms

31
Q

Describe the structure of a covalent compound

A

Simple molecule (one of to atoms)

32
Q

What is a lone pair of electrons?

A

A pair of electrons not involved in bonding

33
Q

What is a dative bond?

+ what is it also know as?

A

A covalent bond where both electrons come from one atom in bond

Co-ordinate bond

34
Q

In displayed formula what is a dative covalent bond shown as?

A

An arrow going from donating to accepting atom

35
Q

What is average bond enthalpy?

A

A measurement of the strength of a covalent bond (higher= stronger)

36
Q

Define metallic bonding

A

The electrostatic force of attraction between a sea of delocalised electrons and the positive nuclei of metal atoms

37
Q

Explain the melting point of a metal

A

High

Strong electrostatic forces of attraction between nuclei and sea of delocalised electrons, lots of energy to overcome

38
Q

Explain the behaviour of a metal when hammered

A

Malleable and ductile

Regular layers, slide over each other and electrons hold new structure in place

39
Q

Define ductility

A

The ability to form a wire ( drawn/stretched into wire)

40
Q

Explain the conductivity of a metal

A

Good conductors of heat and electricity

Charges (electrons) free to move and carry charge

41
Q

What metal is liquid at RT?

A

Mercury

42
Q

What does isoelectric mean?

A

Same number of electrons

Chemistry (28 decks)

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