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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is the goal of elements bonding?

A

To have a full outer shell

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2
Q

How many electrons are in a full outer shell?

A

8 Electrons

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

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3
Q

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

A

They share electrons

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4
Q

What are some properties of Covalent Bonds?

A
  • Liquid or Gas
  • Insoluble
  • Insulative (doesn’t conduct electricity)
  • Low Melting and Boiling Point
  • Brittle (Not Malleable)
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5
Q

Why do atoms want a full outer shell?

A

They become much more stable

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6
Q

What are some examples of a Covalent Bond?

A
  • Water - H2O
  • Carbon Dioxide - CO2
  • Nitrogen - N2
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7
Q

What types of elements are involved in Covalent Bonds?

A

2 Non-Metals

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8
Q

How do elements bond through Ionic Bonding?

A

They give away and recieve electrons

Non-metals recieve electrons, and metals give away electrons

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9
Q

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

A

1 Electron

Remember the 2.8.8 Rule

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10
Q

What is a cation?

A

A postive ion

Metal Atoms are always the cation in an ionic bond

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11
Q

What is an anion?

A

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

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12
Q

What are some properties of an ionic bond?

A
  • 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

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13
Q

Why are Ionic Compounds only conductive when dissolved or melted?

A

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

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14
Q

What are polyatomic ions?

A

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

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15
Q

What is a lattice?

A

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

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16
Q

What are some examples of an Ionic Bond?

A
  • 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

17
Q

What types of elements are involved in Ionic Bonding?

A

1 Metal and 1 Non-Metal

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

18
Q

What is an allotrope?

A

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

19
Q

What characterizes a Giant Covalent Bond?

A

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

20
Q

What are some properties of Diamond?

A
  • 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

21
Q

What are some properties of Graphite?

A
  • 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

22
Q

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

A

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

23
Q

What are some examples of Giant Covalent Bonds?

A
  • Diamond
  • Graphite
  • Fullerene
  • Sand
24
Q

What is the structure of metal bonds?

A

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

25
Q

What are some properties of metallic bonds?

A
  • Solid
  • Insoluble
  • Conducts Electricity
  • High melting and boiling point
  • Malleable (Bendy, Not brittle)
26
Q

What are some examples of Metallic Bonds?

A
  • Gold
  • Silver
  • Iron
  • Copper

All metals that are just by themselves are metallic bonds

Chemistry (6 decks)

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