Grade 9 - Bonding

Question 1

What is the goal of elements bonding?

Answer 1

To have a full outer shell

Question 2

How many electrons are in a full outer shell?

Answer 2

8 Electrons

Hydrogen and Helium are the only elements with 2 electrons in their outer shell

Question 3

How do elements gain a full outer shell with covalent bonding?

Answer 3

They share electrons

Question 4

What are some properties of Covalent Bonds?

Answer 4

• Liquid or Gas
• Insoluble
• Insulative (doesn’t conduct electricity)
• Low Melting and Boiling Point
• Brittle (Not Malleable)

Question 5

Why do atoms want a full outer shell?

Answer 5

They become much more stable

Question 6

What are some examples of a Covalent Bond?

Answer 6

• Water - H2O
• Carbon Dioxide - CO2
• Nitrogen - N2

Question 7

What types of elements are involved in Covalent Bonds?

Answer 7

2 Non-Metals

Question 8

How do elements bond through Ionic Bonding?

Answer 8

They give away and recieve electrons

Non-metals recieve electrons, and metals give away electrons

Question 9

If Fluorine has 9 electrons, how many does it need for a full outer shell?

Answer 9

1 Electron

Remember the 2.8.8 Rule

Question 10

What is a cation?

Answer 10

A postive ion

Metal Atoms are always the cation in an ionic bond

Question 11

What is an anion?

Answer 11

A negative ion

Non-Metal Atoms are always the anion in an ionic bond

also its pronounced like onion definitely mhm i would never lie

Question 12

What are some properties of an ionic bond?

Answer 12

• Solid
• Soluble
• Conductive, only when melted or dissolved1
• High melting and boiling point
• Brittle (Not Malleable)

1E.g salt is only conductive when it is dissolved in water

Question 13

Why are Ionic Compounds only conductive when dissolved or melted?

Answer 13

When they’re solid, the electrons are locked in place by the bonds of the lattice, however these bonds are broken when the compound is dissolved or melted, meaning the electrons can move about freely, and is thus conductive

Question 14

What are polyatomic ions?

Answer 14

Polyatomic ions are ions with more than one atom (what a suprise). They cannot be separated, and whenever there is a change, it applies to all atoms together as a whole

Some examples include Hydroxide (OH-) and Nitrate (NO3 -)

Please look up the actual formulas for the examples, I can’t do the proper small numbers on the formulas

Question 15

What is a lattice?

Answer 15

A lattice is a giant structure formed of repeating cations and anions, which is repeated millions of times. Most Ionic Compounds form these lattices and it results in crystals. (Other ionic compounds that aren’t crystals dont have these lattices, but this isnt that important)

This is the same thing as the Giant Covalent Bonds thingy

Question 16

What are some examples of an Ionic Bond?

Answer 16

• Sodium Chloride - NaCl - Table Salt
• Sodium Bicarbonate - NaHCO3 - Baking Soda
• Sodium Fluoride - NaF - Its the important thing in toothpaste

Salt is the only important one, I just needed more examples lol

Question 17

What types of elements are involved in Ionic Bonding?

Answer 17

1 Metal and 1 Non-Metal

The metal atom becomes a cation and the non-metal atom becomes an anion

Question 18

What is an allotrope?

Answer 18

An allotrope is the different forms of an element, depending on how they atoms are bonded together

E.g. Carbon has various allotropes such as diamond and graphite

Question 19

What characterizes a Giant Covalent Bond?

Answer 19

A giant covalent bond consists of a very large repeating lattice. Depending on the element and allotrope, the pattern of the lattice can differ, and so can the properties

Diamond has a different structure than Graphite, look up the patterns

Question 20

What are some properties of Diamond?

Answer 20

• Each Carbon atom is bonded to 4 others
• Hardest known natural substance (that’s what she said)
• Highest melting point of any element, 3500°C
• Does not conduct electricity
• They are used for their hardness in tools such as drills and saws, because this will keep them sharper and harder for longer. Also used for Jewelery because oooo shiny rock

Diamonds suck for Jewelry because Capitalism lol, if you want shiny rock get sapphire instead, they’re basically identical

Question 21

What are some properties of Graphite?

Answer 21

• Conducts electricity1
• Each Carbon is bonded to 3 others, leaving 1 free
• Is separated into layers, which makes it slippery
• Because of slipperiness, its used for lube lol and also pencils because yes

1 Graphite is like the only Giant Covalent thingy that does this

Question 22

Why is Graphite conductive, but other Giant Covalent Bonds aren’t?

Answer 22

Graphite has a structure that is split into many different layers. These layers are very weakly bonded together, so electrons can move freely between them, and so its conductive

Question 23

What are some examples of Giant Covalent Bonds?

Answer 23

• Diamond
• Graphite
• Fullerene
• Sand

Question 24

What is the structure of metal bonds?

Answer 24

They consist of many cations all connected in a lattice, which are surrounded by a sea of electrons

Question 25

What are some properties of metallic bonds?

Answer 25

• Solid
• Insoluble
• Conducts Electricity
• High melting and boiling point
• Malleable (Bendy, Not brittle)

Question 26

What are some examples of Metallic Bonds?

Answer 26

• Gold
• Silver
• Iron
• Copper

All metals that are just by themselves are metallic bonds