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workbook 2 Flashcards

(63 cards)

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1
Q

what is matter

A

anything that takes up space and has mass

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2
Q

what are the 3 different states of mass

A

solid, liquid and gas

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3
Q

describe a solid

A

particles are in a fixed position close together

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4
Q

describe a liquid

A

particles are free to move and take shape of the container because they’re not held as rigidly and move relative to one another

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5
Q

describe a gas

A

occupies the total space of the container and fills the total volume because the particles are very widely spaced and move independently

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6
Q

compressibility of a solid

A

none

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7
Q

compressibility of a liquid

A

none

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8
Q

compressibility of a gas

A

compressible

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9
Q

diffusion of a solid

A

none

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10
Q

diffusion of a liquid

A

slow

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11
Q

diffusion of a gas

A

fast

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12
Q

what are the 2 types of matter

A

pure substances and mixtures

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13
Q

what are pure substances

A

matter which is homogenous and has definite fixed composition

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14
Q

what are the 2 types of pure substances

A

elements and compounds

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15
Q

can elements be split any further chemically

A

no

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16
Q

what are mixtures

A

2 or more pure substances. The components maintain their own properties and can be separated by physical methods

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17
Q

what are the 2 types of mixtures

A

homogenous and heterogenous

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18
Q

what is a homogeneous mixture

A

Uniform composition and properties throughout

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19
Q

what is a heterogeneous mixture

A

not uniform composition and properties throughout

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20
Q

what are the boiling points like in pure substances

A

well defined and constant
eg. water freezes at 0 and boils at 100

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21
Q

what are the boiling points like in mixtures

A

they vary due to the different compositions in the water

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22
Q

what is the density like of a pure substance

A

fixed and constant throughout

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23
Q

what is the density like of a mixture

A

vary depending on the ratio of different substances through the mixture

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24
Q

what are the properties like of a pure substance

A

constant and well defined

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25
what are the properties like of a mixture
will always vary depending on where its from
26
what are the 2 categories of properties
physical and chemical
27
what are physical properties
determined without changing the chemical composition
28
eg of physical properties
colour, taste, odour, lustre, density
29
what are chemical properties
the ability of the substance to form new substances
30
eg of chemical properties
flammability, toxicity, acidity, reactivity with other substances, and heat of combustion
31
what are the 2 types of changes
physical and chemical
32
what are physical changes
changes in physical properties, they occur without a change to the chemical composition
33
eg of physical changes
cutting paper, melting ice
34
what are chemical changes
new substances with different compositions and properties formed
35
eg of chemical changes
burning wood, digesting food, and cooking an egg
36
physical properties of ionic substances
Hard and brittle Non-conductors in a solid state but good conductors when aqueous High melting and boiling points
37
what are cations
positively charged ions
38
what are anions
negatively charged ions
39
naming ionic compounds
The name of the positive ion is written first. ii. The name of the negative ion is written second and the ending is changed to ‘ide’ eg. Chlorine becomes chloride. iii. Where the ionic compound has water molecules of crystallisation, the number of water molecules is indicated e.g. sodium carbonate-10-water = Na2CO3.10H2O
40
how strong are covalent molecular bonds
weak
41
can covalent bonds conduct electricity
no because the electrons are being shared and there are no free ones to carry the charge
42
naming molecular compounds
The name of the elements closer to the bottom or left hand-side of the periods table is written first ii. The second part of the name is obtained by adding the suffix, ‘ide’, to the stem of the name of the second element. iii. Where a molecule contains more than one atom of one type of the number of atoms is indicated by the prefix's ‘mono’, ‘di’, ‘tri’, ‘tetra’, ‘penta’ and ‘hexa’ which stand for 1, 2, 3, 4, 5 and 6 respectively. The prefix ‘mono’ is not used for the first-named element.
43
what is bonding
the force holding atoms together
44
what is the structure of metallic bonding
Metallic bonding has a sea of delocalised electrons. The valent electrons in metallic bonding are delocalized (not bound to any specific atom) meaning they are free to move through the entire metal structure.
45
how hard are metallically bonded substances
yes because the bonds are strong but not rigid
46
are metallic substances good conductors
the delocalised electrons are free to carry the charge through the whole structure
47
why are metallic substances malleable and ductile
the delocalized electrons allow atoms to slide over one another without disrupting the overall medallic bond
48
what are the melting points of metallic substances
high melting and boiling points because of the strong electrostatic attraction between the positive metal ions and the delocalized electrons
49
what is the structure of ionic bonding
In ionic solids, ions are held in the 3D crystal lattice by the strong electrostatic attraction to the oppositely charged ions around it. They form between a metal and a non-metal ion
50
what are the melting points of ionic bonding and why
high melting and boiling points because the electrostatic attraction between ions is strong
51
are ionic substances conductors?
Non-conductor when solid: no free electrons or ions to conduct charge Conductor when in a solution: free ions to conduct electricity
52
why are ionic substances brittle
hitting the solid may cause movement layers so that positive ions are next to positive ions and negative ions are next to negative ions causing repulsion and shattering
53
why are ionic solids hard
because the bonds are hard and rigid
54
eg of ionic bonding
magnesium sulfate, sodium chloride
55
eg of metallic bonding
iron, copper, titanium (any metal)
56
structure of covalent molecular bonding
Formed when 2 or more atoms share electrons to achieve a more stable electron configuration, often resembling a noble gas configuration. Occurs between 2 non-metal atoms
57
what are the melting points of covalent molecular bonds and why
Low melting and boiling points: bonds between individual molecules (intermolecular bonds) are weak and little energy is required to break the bonds between molecules
58
what are lewis dot diagrams
ways of representing covalent bonds
59
what is the structure of covalent network bonding
They are large, rigid, 3 dimensional arrangements of atoms held together by strong covalent bonds
60
what is the melting point of a covalent network bond and why
High melting and boiling points: there are millions of strong bonds, so a lot of energy is needed to break all of them.
61
are covalent network bound substances conductors
no because there are no free electrons to carry charge
62
why are covalent network bound substances hard and brittle
the electrostatic attraction between atoms and bonded electrons are very strong
63
eg of covalent network bonds
diamond, silica

CHEM (6 decks)

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