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Chem > Chap 2 - Ionic, covalent, metallic, giant covalent > Flashcards

Chap 2 - Ionic, covalent, metallic, giant covalent Flashcards

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1
Q

define aqueous

A

dissolved in solution

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2
Q

define molten

A

melted

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3
Q

what are 2 types of mobile charge carriers

A

-ions
-electrons

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4
Q

define lattice

A

regular arrangement of alternating positive and negative ions.

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5
Q

Which diagram is used in ionic and simple covalent bonding

A

dot and cross

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6
Q

define an ionic bond

A

transfer of electrons between positive metal ions and negative non metal ions

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7
Q

What holds an ionic bond together

A

electrostatic forces of attraction between positive metal ions and negative non metal ions

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8
Q

Metals lose electrons to? (ionic)

A

form positive ions

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9
Q

non metals gain electrons to?(ionic)

A

form negative ions

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10
Q

which shell is the electron lost from or added to

A

valance shell

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11
Q

what must the electrical configuration of ions have

A

all shells must be full

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12
Q

if 2 diff atoms of same element have the same electronic configuration as ions, are they the same?

A

no because the proton numbers are diff.

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13
Q

how is the subscript of an element diff to the number in front of the element

A

subscript- there are that certain numbers of elements in the molecule
in front of element- there are that number of molecules

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14
Q

when explaining the dot and cross of an ionic bond what are the 4 things needed to say

A

-total number of electrons in each element and in each shell
-how much electron needed to fill the valance shell of the element
-therefore, how many atoms are needed
-gained = positive metal ions
lost = negative non metal ions

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15
Q

what is the structure in an ionic bond

A

lattice

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15
Q

explain the melting and boiling point of an ionic bond

A

high because the strong electrostatic forces of attraction between positive metal ions and negative non metal ions require a lot of energy to overcome

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15
Q

explain when and how electricity is conducted in an ionic bond

A

only when aqueous or molten because that is when the ions are mobile and can carry charge through the structure

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16
Q

when writing the dot and cross of ions on the electrons transferred, what goes first- number or charge

A

number
eg, 2+

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17
Q

when finding the number of atoms needed in an ionic dot and cross, what must you try to find

A

LCM of the numbers of electrons needed by the non metal and metal

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18
Q

define / describe metallic bond

A

a lattice of positive metal ions in a ‘sea’ of delocalised electrons held by electrostatic forces of attraction

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19
Q

what is the structure in an metallic bond

A

lattice

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20
Q

what holds metallic bonds together

A

electrostatic forces of attraction between positive metal ions and a ‘sea’ of delocalised electrons

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21
Q

are metallic bonds good conductors of heat and electricity

A

yes. they have delocalised electrons which are mobile and can carry charge or heat energy through the structure.

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22
Q

explain the melting and boiling point of metallic bonds

A

high, strong electrostatic forces of attraction between positive metal ions and a ‘sea’ of delicalised electrons require a lot of energy to overcome

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23
Q

explain the malleability of metallic bonds

A

they are malleable, metals have a regular structure with layers that can slid off each other

24
Q

name the 9 properties of metals

A

-good conductors of heat
-good conductors of electricity
-ductile
-malleable
-some are magnetic (iron, cobalt, nickel)
-high melting and boiling points (usually solids at room temp. except mercury)

25
Q

define ductile

A

can be drawn into wires

26
Q

define malleable

A

can be bent or hammered into shape

27
Q

which metals are magnetic

A

iron, cobalt, nickel

28
Q

define volatile

A

turns into gas easily

29
Q

when explaining a propriety of an molecule, what must you say at first about it

A

the type of bond it is

30
Q

define a covalent bond

A

shared pair of electrons between non metals

31
Q

what are the 2 types of covalent bonds

A

simple covalent, giant covalent

32
Q

what is the structure of simple covalent bonds

A

small molecules

33
Q

what is the structure of giant covalent bonds

A

lattice

34
Q

what holds simple covalent bonds together

A

-many strong covalent bonds (intramolecular forces of attraction) between atoms
-intermolecular forces of attraction between molecules

35
Q

what holds giant covalent bonds together

A

MANY strong covalent bonds (intramolecular forces of attraction) in between atoms

36
Q

does giant covalent bonds have intermolecular forces of attraction

A

no

37
Q

which forces are weakened or broken when heating

A

intermolecular forces of attraction

38
Q

what do you need to think about when drawing dot and cross of simple covalent

A

-number of electrons in valance shell of each element
-number of electrons needed

39
Q

how do you show the number of bonds in a displayed formula for simple covalent

A

the number of dashes

40
Q

H2, Cl2, M2O, CH4, NH3, HCL, CH30H- single bonds
C2H4, O2, CO2- double bonds
N3- triple bond

A

remember the structure for CH3OH-
H
|
H - C - O - H
|
H

41
Q

explain the melting and boiling point of simple covalent bonds

A

low, the weak intermolecular forces of attraction between molecules require little energy to overcome

42
Q

can simple covalent structure conduct electricity

A

no, there are no mobile charge carriers

43
Q

name 2 giant covalent structures

A

diamond, graphite

44
Q

explain the melting and boiling point of giant covalent bonds

A

high, there are MANY strong covalent bonds in between atom which require a lot of energy to overcome

45
Q

list the physically properties of diamond

A

-hard (cant be scratched easily)
-high melting and boiling points
-no electricity conduction
-shiny

46
Q

list all the important notes on diamond

A

-hard (cant be scratched easily)
-high melting and boiling points
-no electricity conduction
-shiny
-used as a cutting tool
-has MANY strong covalent bonds
-each carbon atom is bonded to 4 other carbon atoms

47
Q

list the physically properties of graphite

A

-soft and slippery
-high melting and boiling point
-can conduct electricity
-dull

48
Q

list all the important notes on graphite

A

-soft and slippery
-high melting and boiling point
-can conduct electricity
-dull
-used as a lubricant
-has MANY strong covalent bonds
–each carbon atom is bonded to 4 other carbon atoms (so 1 delocalised electron)
-has layers

49
Q

what is the structure of giant covalent

A

lattice

50
Q

what must you add when describing bonds in a giant covalent structure

A

many

51
Q

can giant covalent structures conduct electricity

A

only graphite because graphite has delicalised electrons which are moblile and can carry charge through the structure

52
Q

what is the solubility of covalent compounds

A

low, they do not dissolve in water easily

53
Q

what is the volatility of covalent compounds

A

high, they turn into gas easily.

54
Q

properties of ionic bonds

A

-Low volatility
-high solubility
-high melting and boiling point
-conducts when molten or aqueous

55
Q

describe ionic bonds

A

electrostatic attraction between positive metal ions and negative non-metal ions

56
Q

why does bromine have a low boiling point

A

-bromine is a covalent bond
-bromine is non-metal
-it requires little energy to overcome intermolecular forces of attraction btw molecules.

57
Q

solubility of covalent compounds

A

low, covalent compounds cannot dissolve easily in water.

58
Q

volatility of covalent compounds

A

high, they have low melting and boiling points.

Chem (12 decks)

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