Bonding, Structures And Properties Flashcards

1
Q

what is an isotope

A

any of two or more forms of an element, that have the same number of protons and the same atomic number, but having different numbers of neutrons and therefore different atomic weights.
so they have the same chemical properties but different physical properties.

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2
Q

what is an ionic bond?

A

ionic bonds are formed between a metal and a non-metal. the metal loses electrons from its outer shell you form positive ions and the non-metal gains electrons to form negative ions.

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3
Q

what happens as the group number increases in the periodic table? ( more in outer shell)

A

there are more elections in the outer shell so the less reactive they get.

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4
Q

what happens to reactivity as you go down the groups?

A

They get more reactive as you go down because the outer electrons are further away from the nucleus

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5
Q

what is a covalent bond?

A

it is between two non-metals and they share the electrons instead of giving and taking.
e.g water

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6
Q

in the periodic table,
what us the top number?
what is the bottom number?

A

top=mass number

bottom=atomic number

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7
Q

what is the structure of an ionic compound?

A

a huge lattice of positive and negative ions packed together in a regular arrangement.

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8
Q

what are 3 properties of ionic compounds?

and why?

A

HARD SUBSTANCE- they consist of a regular pattern of opposite ly charges ions with strong bonds between them.
BRITTLE- any small distortion of crystal brings ions with the same charge together. Same charges repellent so the crystal splits apart.
HIGH MELTING POINT- due to strong forces of attraction holding the latuce together.

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9
Q

what factors affect the strength of an ionic bond and thus it’s melting point?

A

attractive forces are stronger between certain atoms and compounds if they have a higher charge (2+) than (1+)

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10
Q

why do most ionic compounds dissolve in water?

A

because water molecules are able to break down the ionic bonds between the opposite ly charged ions

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11
Q

why do ionic compounds in the solid state not conduct electricity.

A

the ions are held in a fixed position by strong forces of attraction.

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12
Q

why do ionic compounds in a molten state or aqueous solution conduct electricity

A

the ions are free to move and carry charge

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13
Q

what happens to the rate or reaction if you increase the surface area?

A

it will increase, as it gives particles a bigger area of solid reactant to react with.

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14
Q

what happens when a catalyst is added? and why?

A

it speeds up the reaction but is itself chemicals unchanged at the end. as the catalyst provides an alternative pathway for a reaction with a lower ‘EA’ (activation energy).

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15
Q

if you increase the pressure of a gasses reaction what happens to the rate of reaction? and why?

A

the rate or reaction increases, as there are more particles in a given area, so more chance of successful collisions.

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16
Q

what is a potential problem of using a catalyst in industrial processes?

A

it adds an extra step that is to separate the catalyst after.

17
Q

what is the method to show that the solid acted as a catalyst and not as a reactant?

A
  1. weigh the solid.
  2. use the solid.
  3. filter, wash and dry Tehran solid.
  4. rewaigh the solid.
  5. re-use the solid.
18
Q

why do ionic compounds have a high melting point?

A

very strong electrostatic forces of attraction between opposite charged ions which require a lot of energy to overcome.

19
Q

what is a simple molecular structure?

A

two or more atoms covalently bonded together in a small group. most non-metals are a simple molecular

20
Q

what is the structure of a simple molecular structure?

A

strong covalent bonds between atoms, weak intermolecular forces between molecules.

21
Q

what are some properties of a simple molecular structure?

A

-it is an insulator because the outer electrons of bonded atoms are all involved in bonding and are not free to move.

22
Q

why do metals conduct electricity?

A

they have demoralised electrons cat can move throughout the structure and carry charge.

23
Q

why are metals maluble?

A

the metal atoms (cations) are arranged in layers that can slide over eachother.

24
Q

what is a metallic bond?

A

the strong electrostatic forces of attraction between the positive cations and the delocalised electrons.

25
Q

structure of metals?

A

giant 3D lattices

delocalised electrons

26
Q

why do covalent molecules have low melting and boiling points?

A

the interview molecular forces are weak and do not take very much heat energy to break.

27
Q

do simple covalent molecules conduct electricity?

A

no, the molecules do not have any over all electrical charge and there are NO electrons mobile enough to move from molecule to molecule and carry charge.

28
Q

what is a bucky ball?

A

C(60) a molecule made of 60 carbon atoms.

29
Q

in terms of its structure, why does magnesium oxide have a very high melting point?

A

it is a giant structure with strong electrostatic forces of attraction between oppositly charged ions.

30
Q

what is an ionic compound?

A

a chemical compound composed of ions held together by electrostatic forces of attraction

31
Q

what types of bonds are in a aimple molecular structure?

A

covalent

32
Q

which bonds use electrostatic forces of attraction?

A

metallic and ionic

only if a metal is present

33
Q

what are the 2 types of covalent structure?

A
  • macromolecular.

- simple molecular.

34
Q

what is a macro molecular structure?

A

many atoms covalently bonded to form an infinate structure.

35
Q

what are 3 examples of a macromolecular structure?

A
  • diamond
  • silicon dioxide
  • graphite
36
Q

what is a macro molecular structure’s melting point like?

A

high as it has many strong covalent bonds.

37
Q

out of graphite, diamond and silicone dioxide which conduct electricity and which are insulators?

A

graphite conducts as it has delocalised electrons but diamond and silicone dioxide are insulators because there are no delocalised electrons.