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GCSE Chemistry > C2.2 - Bonding > Flashcards

C2.2 - Bonding Flashcards

1
Q

What is the relative atomic mass (RAM or Ar)

A

the number of protons and neutrons in an atom (mass number). the unit for RAM are atomic mass units (a.m.u)

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2
Q

what is the relative molecular mass ( Mr or RMM)

A

the numebr of protons and neutrons in a molecule

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3
Q

what is the realtive formula mass (Mr or RFM)

A

the number of protons and neutrons in a formula

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4
Q

what is the empirical formula

A

the empirical formula is the simplist whole number ratio of each type of atom in a compound

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5
Q

how can empirical formula be calculated

A

empirical formula can be calculated from the number of atoms present or by converting the mass of the element or compound

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6
Q

what is bonding

A

bonding is an attraction between atoms in elements and compounds

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7
Q

what are some examples of metals

A

aluminium, lithium, rhodium, gallium

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8
Q

what are some physical properties of metals

A

metals are good conductors of heat and electricity. metals are dense, ductile, shiny and hard. metals have high melting/boiling points

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9
Q

what are some chemical properties of metals

A

metals form ionic compounds. metals lose electrons to form mwtal cations. metals react with oxygen to produce oxides. metals react with acids to produce salt and hydrogen

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10
Q

what are some examples of non metals

A

fluorine, sulphur, nitrogen,hydrogen

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11
Q

what are some physical properties of non metals

A

non metals are brittle when solid. non metals are poor conductors of electricity. non metals have low melting/boiling points. non metals are brittle when solid

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12
Q

what are some chemical properties of non metals

A

non metals form covalent bonds with other non metals, non metals form ionic bonds with metals

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13
Q

where are the outermost electrons found in metals

A

in metals, the outermost electrons are found between the positive particles

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14
Q

what are ions

A

ions are charged particles (positive or negative)

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15
Q

how do ions form

A

ions form when electrons are transferred from a metal to a non metal

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16
Q

what are anions

A

anions are ions with a negative charge acquired from gaining an electron or electrons

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17
Q

what are cations

A

cations are ions with a positive charge acquired from losing an electron or electrons

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18
Q

are metal ions positive or negative

A

metal ions are positive

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19
Q

what do non metal ions form

A

non metal ions form negative ions

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20
Q

what are ionic bonds

A

ionic bonds are the electrostatic forces of attraction that hold the ions together

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21
Q

how is an ionic bond formed

A

an ionic bond is formed when one or more electrons are donated by one atom or molecule and recieved by another atom or molecule

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22
Q

how is an ionic compound formed

A

When a metal element reacts with a non-metal element

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23
Q

what happens to the ions if an ionic compound is in a solution or in a molten state

A

if an ionic compound is in a solution or in a molten state the ions move freely

24
Q

what happens to the ions if an ionic compound is solid

A

if an ionic compound is solid, the ions are arranged in a way to cancel out the charges

25
what compounds have ionic bonds in them
compounds with a metal and a non metal have ionic bonds in them
26
why do ionic bonds form
ionic bonds form due to the attraction between the positive and negative ions
27
do ionic bonds have a high or low melting/boiling points
ionic bonds have a high melting/boiling points
28
when can ionic compounds conduct electricity
ionic compounds can conduct electricity when they are molten and in solution
29
what are some properties of ionic compounds
ionic compounds contin a metal and a non metal in the same molecule. some ionic compounds dissolve (in water). some ionic compounds are insoluble. they are strong
30
how is a covalent bond formed
a covalent bond is formed when atoms share electrons to complete their outermost shell
31
what is a covalent bond
when the shared pair of electrons join the atoms together
32
what are simple covalent molecular structures
simple covalent molecular structures are covalent molecules that contain only a few atoms
33
do simple covalent molecular structures have low or high melting/boiling points
simple covalent molecular structures have low melting/boiling points
34
what are simple covalent molecular structures at room temperature
simple covalent molecular structures are liquids and gases at room temperature
35
what forms crystals at room temperature
ionic compounds such as sodium chloride form crystals at room temperature
36
what are some properties of covalent bonds
covalent bonds form between non metals and non metals. covalent bonds share electrons (to complete outer shell). covalent bonds can be found in water, methane, carbon dioxide, hydrogen and chlorine molecules
37
why are models of bonding used
models are used to show how atoms are bonded together
38
what can dot and cross diagrams show
dot and cross diagrams can show: 1) each shell of electrons or just the outer shell. 2) how electrons are donated or shared
39
what is an example of a covalent compound
methane - methane is a covalent compound
40
what do ball and stick models show
ball ans stick models give an idea of the 3D shape of a molceule or compound
41
what are some limitations of models of bonding
1) the scale of the nucleus to the electrons is wrong in most models. 2) models show bonds as physical structures. 3) most modelns don't give an accurate idea of the 3D shape of a molecule. 4) the bond lengths are not in propotion to the size of the atoms
42
what are simple molecules
simple molecules are when non metals or non ionic molecules join together, the atoms share electrons are form a covalent bond
43
what is an example of a covalent molecule
hydrogen gas
44
when are giant covalent structures formed
giant covalent structures are formed when the atoms of a substance form repeated covalent bonds. an exmaple is silicon dioxide
45
when is a polymer formed
a polymer is formed when repeated units are covalently bonded together. an example is when lots of ethene molecules are joined together they form poluethene
46
how are metal atoms held together
metal atoms are held together by strong metallic bonds
47
how do metals become positively charged
the metals become positively charged when the metal atoms lose their outermost electrons
48
how is a sea of delocalised (free) electrons formed
a sea of delocalised (free) electrons is formed because electrons can move freely from one metal ion to another
49
what does an element contain
an element contains one type of atom
50
what cannot be chemically broken down into simpler substances
elements cannot be chemically broken down into simpler substances
51
how many naturally occuring elements are there
there are about 100 naturally occurring elements
52
who developed the design of the modern periodic table
the design of the modern period table was first developed by Mendeleev
53
In Mendeleev's table, what were the elements (placed into groups) based off of
In Mendeleev's table, the elements were placed into groups based on their atomic mass w
54
In Mendeleev's table, why were some elements put into the wrong places
some elements were put into the wrong places because the values used for their atomic mass were incorrect
55
what does the modern periodic table take into account
the modern periodic table takes into account the arrangement of electrons, the number of electrons in the outermost shell, and atomic number
56
what is a group, in the periodic table
a group is a vertical column of elements
57
what is a period, in the periodic table
a period is a horizontal row of elements

GCSE Chemistry (12 decks)

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