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Chemistry > Bonding, Structure and properties and matter > Flashcards

Bonding, Structure and properties and matter Flashcards

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1
Q

When are ions made

A

When electrons are transferred

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2
Q

Why do atoms lose/ gain electrons

A

To gain full outer shells

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3
Q

What groups are most likely to form ions

A

1,2 (lose electrons to make positive) and 6,7 (gain electrons to make negative)

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4
Q

Explain ionic bonding

A

When a metal and a non metal react together. The metal loses electrons to form a positive ion and the non metal gains electrons to form a negative ion. The oppositely charges ions are attracted by strong electrostatic forces in an ionic bond

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5
Q

What type of structure are ionic compounds

A

Giant ionic lattice- organised regularly

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6
Q

Prooperties of ionic compounds

A
  • High melting/ boiling points
  • Can’t carry charges unless molten
  • Some ionic compounds dissolve in water so they’ll carry electric charge
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7
Q

What is empirical formula

A

The simplest ratio of atoms in an element in whole numbers

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8
Q

Explain covalent bonding

A

Non metals bond with covalent bonding
Positively charged nucleus of atoms are attracted two shared pairs of electrons, with electrostatic forces- strong bonds
- Each covalent bond provides an extra electron for each atom

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9
Q

What is the display formula

A

The one with the letters and sticks connecting them

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10
Q

What are covalently bonded substances often labelled

A

Simple molecular substances

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11
Q

Properties of covalently bonded substances

A
  • Low melting/ boiling point as there are weak intermollecular forces
  • Often liquids/ gases at room temperature
  • As molecules get bigger, the strength of intermolecular forces get bigger so they have higher melting/ boiling points
  • Don’t conduct electricity
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12
Q

What is a polymer

A

A long chain of a repeating unit

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12
Q

What is different in giant covalent structures to simples and what effect does that have on melting point

A

In giant covalent structures, all of the atoms are bonded, which means the melting points are very high

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13
Q

Structure of diamonds

A

Giant covalent- all carbon atoms are bonded to 4 other atoms

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14
Q

Strucure of graphite

A

Each carbon is bonded to 3 others and there is one delocalised electron

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15
Q

Properties of diamond and why (2)

A
  • Each carbon is bonded to 4 others- which means it is hard
  • Doesn’t conduct electricity because there are no free electrons
16
Q

Properties of graphite and why

A
  • No bonds between layers so they can easily slip over each other
17
Q

What is a fullerene

A

A sphere of carbon

18
Q

Uses of fullerenes (4)

A
  • Can be used to ‘cage’ other molecules so they can be used to deliver drugs into bodies
  • Can form nanotubes
  • Have high tensile strength (don’t break when stretched)
  • Conducts thermal and electrical energy
19
Q

Explain metallic bonding

A
  • Electrons in the outer shell of metals mean that the metals form positive ions
  • The sea of delocalised electrons and positive metal ions have large electrostatic forces of attraction
  • Delocalised electrons hold together the lattice
20
Q

Properties of metals (3)

A
  • Solid at room temperature
  • Good conductors of electricity and heat
  • Most metals are malleable
21
Q

Why are alloys harder than pure metals

A

Different sized atoms distort the layers of metal atoms making it more difficult for the to slide over each other so the metal is harder

22
Q

What are the 3 states of matter

A

Solid liquid gas

23
Q

Properties of solids (3)

A
  • Strong forces which hold particles in fixed positions in a regular arangement
  • Particles dont move from their positions
  • The otter solids get, the more they vibrate
24
Q

Properties of liquids (2)

A
  • Weak forces of attraction between particles so they are free to move past each other
  • Dont have a definite shape
25
Q

Properties of gas (3)

A
  • 1 mole of gas is always 24dm^3 at 1 ATM
  • Always fit the container they’re in
  • Particles move in a constant random motion
26
Q

What do these mean in a substance equation
(s)
(l)
(g)
(aq)

A

Solid
Liquid
Gas
Dissolved in water

27
Q

Explain how a substance going from solid to liquid to gas via heating

A
  • When a solid is heated, the particles gain more energy
  • They eventually get enough energy to break free from their positions in melting and they turn to a liquid
  • When a liquid is heated, it gains more energy
  • Particles vibrate faster and break the bonds holding them together
  • This is called evaporation and the liquid becomes gas
28
Q

Explain how a substance goes from gas to solid

A
  • As the gas cools, the particles no longer have enough energy to overcome the forces of attraction between them
  • Bonds form between particles
  • At the boiling point, so many bonds form that the gas condenses and becomes a liquid
  • When a liquid cools the particles have less energy, so they move around less
  • There’s not enough energy so strong bonds form between them
  • So many bonds form between the particles so they’re held in place and are frozen
29
Q

What is nanoparticles SA to volume ratio and why

A

They have a large SA to colume ratio. As particles decrease in size their surface area increases relative to their volume

30
Q

Why are nanoparticles having a high SA:V ratio good

A

Becuase less of it can be used for catalysts

31
Q

Uses for nanoparticles (4)

A
  • Good for catalysts
  • Could deliver drugs
  • Silver nanoparticles hace antibacterial propertiesso they are added to surgical masks and deodrants
  • Can be used in cosmetics
32
Q

What are some limitations of using nanoparticles (4)

A
  • Effect on health isn’t fully understood
  • Long term impact on health isn’t understood
  • Could damage cells
  • Could harm the environment

Chemistry (10 decks)

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