Electrons, Bonding And Structure

Question 1

What are the blocks in the periodic table called?

Answer 1

S, d, p, f

Question 2

How can you tell a covalent bond is present?

Answer 2

Hydrolysed by water

Liquid at rt

Question 3

How are electrons arranged in an atom?

Answer 3

Around nucleus in shell.

Shell/sub shell/orbital

Question 4

What happens to the energy of shells around the nucleus?

Answer 4

Further away= higher energy

Question 5

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

Answer 5

(n)

Measure of energy of shells

Question 6

What is an orbital?

Answer 6

Region around nucleus that can hold up to 2 electrons

Question 7

What is a sub shell?

Answer 7

Orbitals of same shape grouped together

Question 8

What is a shell/energy level?

Answer 8

Different sub shells grouped together

Question 9

Describe the s subshell

Answer 9

Spherical shape

One orbital

2 electrons max

Starts in first subshell

Question 10

Describe p subshell

Answer 10

Dumbbell shape

3 orbitals (90 degrees to each other)

6 electrons max

Starts in second subshell

Question 11

Describe d subshell

Answer 11

Five orbital

10 electrons max

Starts in third subshell

Question 12

Describe f subshell

Answer 12

7 orbital

14 electrons max

Starts in fourth subshell

Question 13

What is spin pairing and what is it represented by?

Answer 13

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

Shown by arrows

Question 14

What are the electron configuration rules?

Answer 14

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)

Question 15

What is Aufbau’s principle?

Answer 15

Lowest available energy level is occupied first

Question 16

What is Hund’s rule?

Answer 16

Electrons stay impaired for as long as possible in each subshell

Question 17

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

Answer 17

S= left

D= middle

P=right

F= bottom

Question 18

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

Answer 18

Signify the last subshell with an electron in

Question 19

How does chromiums electron configuration end?

+why

Answer 19

3d5 4s1

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

Question 20

How does coppers electron configuration end?

+why?

Answer 20

3d10 4s1

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

Question 21

Why is 4s filled and empties before 3d?

Answer 21

When empty 4s has lower energy than 3d.

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

Question 22

What is an ionic bond?

Answer 22

The electrostatic force of attraction between positive and negative ions

Question 23

What are positive ions also know as?

Answer 23

Cations

Question 24

What are negative ions also know as?

Answer 24

Anions

Question 25

What is the structure of an ironically bonded compound ?

Answer 25

Giant ionic lattice Giant=continually repeating units Lattice =ions packed alternatingly

Question 26

Explain the melting and boiling points of ionic compounds

Answer 26

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

Question 27

Explain the solubility of ionic compounds

Answer 27

Soluble in polar solvents = poles attract ions insoluble in non-polar solvents (hydrocarbons)

Question 28

Explain the conductivity of ionic compounds

Answer 28

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

Question 29

Explain the behaviour of ionic compounds when hammered

Answer 29

Brittle and easily cleaved Layers distort when hammered, like charges align and repel.

Question 30

Define covalent bonding

Answer 30

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

Question 31

Describe the structure of a covalent compound

Answer 31

Simple molecule (one of to atoms)

Question 32

What is a lone pair of electrons?

Answer 32

A pair of electrons not involved in bonding

Question 33

What is a dative bond? + what is it also know as?

Answer 33

A covalent bond where both electrons come from one atom in bond Co-ordinate bond

Question 34

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

Answer 34

An arrow going from donating to accepting atom

Question 35

What is average bond enthalpy?

Answer 35

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

Question 36

Define metallic bonding

Answer 36

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

Question 37

Explain the melting point of a metal

Answer 37

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

Question 38

Explain the behaviour of a metal when hammered

Answer 38

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

Question 39

Define ductility

Answer 39

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

Question 40

Explain the conductivity of a metal

Answer 40

Good conductors of heat and electricity Charges (electrons) free to move and carry charge

Question 41

What metal is liquid at RT?

Answer 41

Mercury

Question 42

What does isoelectric mean?

Answer 42

Same number of electrons