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Chemistry > Bonding, structure, and the properties of matter > Flashcards

Bonding, structure, and the properties of matter Flashcards

1
Q

What are the three types of strong chemical bonds?

A

metallic, ionic and covalent

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2
Q

what is ionic bonding?

A

bond between a metal and a nonmetal they lose electrons to become stable

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3
Q

what is covalent bonding?

A

a bond that forms when two non-metal atoms share a pair of electrons

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4
Q

What is metallic bonding?

A

bond between two metals
delocalised electrons are free to move within the structure

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5
Q

How to work out the charge on the ions of elements in groups 1,2,6 and 7?

A

use the periodic table

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6
Q

How do you draw dot and cross diagrams?

A

element with a circle round it then dots and crosses to show electrons

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7
Q

Describe the structure of a giant lattice (reference forces)

A

strong electrostatic forces of attraction acting in all directions between the oppositely charged ions

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8
Q

What are the limitations of using dot and cross diagrams?

A

doesn’t show the 3D arrangement of the atoms and electron shells

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9
Q

What are the limitations of using ball and stick diagrams?

A

doesn’t show relative size of atoms and bonds

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10
Q

What are the limitations of using 2D diagrams?

A

does not show where ions are located on other layers

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11
Q

What are the limitations of using 3D diagrams?

A

not to scale

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12
Q

What are the different covalent substances?

A

some have small molecules and some have large molecules such as polymers and some have giant covalent structures such as diamonds and silicon dioxide

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13
Q

Describe the structure of a metallic lattice (reference positive ions and electrons)

A

the electrons leave the outer shell of metal atoms forming positive metal ions. the structure of the solid metal consists of closely packed metal ions arranged in a regular way.

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14
Q

Describe the particle model

A

the arrangement and movement of particles in solids liquids and gases

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15
Q

Describe the three states of matter using the particle model

A

solid - closely packed and vibrate
liquid - slightly more loosely packed and move in a fluid motion
gas - spaced out and don’t touch

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16
Q

explain changes in state using the particle model

A

chemical bonds between the particles form break or stretch

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17
Q

What determines melting and boiling point of different substances? (reference forces, particles, bonding and structure)

A

the stronger the forces between the particles the higher its melting and boiling points

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18
Q

What are the limitations of the particle theory in relation to changes of state?

A

It assumes that particles are the same in any substance so cannot adapt to mass or size or force of attraction to other particles.

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19
Q

What are the four state symbols and what do they mean?

A

S = solid
L = liquid
G = Gas
AQ = aqueous

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20
Q

Describe the structure of giant ionic lattice (reference to ions and electrostatic forces)

A

Regular arrangement of alternating positive and negative ions in a 3D shape.

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21
Q

What do ionic compounds have?

A

high melting and boiling points

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22
Q

What do ionic compounds not do when solid?

A

they don’t conduce electrify when solid but they do when melted or dissolved

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23
Q

What do substances which consist of small moles (gases or liquids) usually have?

A

relatively low melting and boiling points

24
Q

What happens when small molecules melt or boil? (reference intermolecular forces present)

A

Weak intermolecular forces are overcome. Covalent bonds are not broken

25
Q

How do intermolecular forces change as the size of the molecules increase and what effect does this have on the melting and boiling point of substances?

A

The bigger the molecule, the bigger its electron cloud meaning the greater the opportunity for intermolecular force.

26
Q

What do small molecules not do?

A

they don’t conduct electricity

27
Q

What are the properties of small molecules in terms of their structure and bonding?

A

strong covalent bonds that hold the atoms together

28
Q

What do polymers have?

A

very large molecules
those molecules are linked to other atoms by strong covalent bonds

29
Q

What is the relative strength of the intermolecular forces between polymer molecules and what effect does this have on their state at room temp?

A

strong compared to the intermolecular forces between smaller molecules

30
Q

What do substances that consist of giant covalent structures have?

A

very high melting points

31
Q

What are giant covalent structures linked by?

A

very strong covalent bonds

32
Q

What are the properties of giant covalent structures in terms of their structure and bonding?

A

high melting point as it takes a lot of energy to break the strong covalent bonds between the atoms
they cannot conduct electricity as they have no overall charge

33
Q

What happens to giant covalent structures when they melt or boil? (reference covalent bonds present)

A

large amounts of energy are needed to overcome their strong covalent bonds to make them melt or boil

34
Q

What are some examples of giant covalent structures?

A

diamond, graphite and silicon dioxide

35
Q

What do metals have?

A

giant structures of atoms with strong metallic bonds

36
Q

What do metallic bonds mean?

A

most have high melting and boiling points?

37
Q

Whats the arrangements of atoms in pure metals?

A

neat layers

38
Q

What are the properties of metals in terms of their structure and bonding?

A

arranged in a regular pattern and are closely packed together

39
Q

What is an alloy and how are the atoms arranged?

A

Atoms of different sizes, this distorts the layers.

40
Q

What are metals good conductors of?

A

electricity and thermal energy

41
Q

Describe the structure of a diamond

A

giant covalent structure in which each carbon atom is joined to 4 other carbon atoms by strong covalent bonds

42
Q

What are some properties of diamonds in terms of its structure and bonding?

A

very hard
very high melting point
^ ( strong covalent bonds)
doesn’t conduct electricity ( no free carbon bond)

43
Q

Describe the structure of graphite?

A

layers of carbon atoms arranged in 6 membered hexagonal rings
each carbon atom forms 3 covalent bonds with other carbon atoms leaving one free bond

44
Q

what are properties of graphite in terms of its structure and bonding?

A

soft and slippery (organised in layers)
high melting point (strong covalent bonds)
Conducts electricity (free carbon bond)

45
Q

Describe the structure of graphene

A

a single layer of carbon atoms tightly bound in a hexagonal honeycomb lattice

46
Q

What do the properties of graphene make it useful for?

A

electronics and composites

47
Q

What are the properties of graphene in terms of its structure and bonding?

A

very high melting point and very strong because of its large regular arrangement of carbon atoms joined by covalent bonds

48
Q

Describe the structure of fullerenes

A

composed entirely of carbon

49
Q

What was the first fullerene to be discovered?

A

Buckminsterfullerene ( sphere shape )

50
Q

What do the properties of fullerenes make theme useful for?

A

nanotechnology, electronics and materials

51
Q

What does nano science refer to?

A

structure that are 1-100nm in size

52
Q

As the side of a curb decreases by a factors of 10 what happens?

A

the surface area to volume ratio increases by a factor of 10

53
Q

Why do nano particles have properties different from those with the same materials?

A

high surface area over volume ratio

54
Q

What do nano particles have?

A

applications in medicine, electronics, cosmetics, suncreams, deodorants and catalysts

55
Q

What are advantages and disadvantages of the applications of nano particle materials?

A

offers the potential for newer faster kinds of computers, more efficient power sources and lifesaving medical treatments
economic disruption and possible threats to security, privacy, health and the environment

56
Q

What are the possible risks associated with the use of nano particles?

A

if you inhale them it may cause lung inflammation and heart problems

Chemistry (10 decks)

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