Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

GCSE Chemistry > C2.2 - Bonding > Flashcards

C2.2 - Bonding Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards GCSE Religious Studies - Edexcel Route A flashcards GCSE Religious Studies - Eduqas Route A flashcards GCSE Geography - AQA flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards GCSE Religious Studies - Edexcel Route B flashcards GCSE Religious Studies - Eduqas Route B 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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what is the relative molecular mass ( Mr or RMM)

A

the numebr of protons and neutrons in a molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is the realtive formula mass (Mr or RFM)

A

the number of protons and neutrons in a formula

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what is bonding

A

bonding is an attraction between atoms in elements and compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what are some examples of metals

A

aluminium, lithium, rhodium, gallium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what are some examples of non metals

A

fluorine, sulphur, nitrogen,hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

where are the outermost electrons found in metals

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what are ions

A

ions are charged particles (positive or negative)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

how do ions form

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what are anions

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what are cations

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

are metal ions positive or negative

A

metal ions are positive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what do non metal ions form

A

non metal ions form negative ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what are ionic bonds

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

how is an ionic compound formed

A

When a metal element reacts with a non-metal element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
Q

what compounds have ionic bonds in them

A

compounds with a metal and a non metal have ionic bonds in them

26
Q

why do ionic bonds form

A

ionic bonds form due to the attraction between the positive and negative ions

27
Q

do ionic bonds have a high or low melting/boiling points

A

ionic bonds have a high melting/boiling points

28
Q

when can ionic compounds conduct electricity

A

ionic compounds can conduct electricity when they are molten and in solution

29
Q

what are some properties of ionic compounds

A

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
Q

how is a covalent bond formed

A

a covalent bond is formed when atoms share electrons to complete their outermost shell

31
Q

what is a covalent bond

A

when the shared pair of electrons join the atoms together

32
Q

what are simple covalent molecular structures

A

simple covalent molecular structures are covalent molecules that contain only a few atoms

33
Q

do simple covalent molecular structures have low or high melting/boiling points

A

simple covalent molecular structures have low melting/boiling points

34
Q

what are simple covalent molecular structures at room temperature

A

simple covalent molecular structures are liquids and gases at room temperature

35
Q

what forms crystals at room temperature

A

ionic compounds such as sodium chloride form crystals at room temperature

36
Q

what are some properties of covalent bonds

A

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
Q

why are models of bonding used

A

models are used to show how atoms are bonded together

38
Q

what can dot and cross diagrams show

A

dot and cross diagrams can show: 1) each shell of electrons or just the outer shell. 2) how electrons are donated or shared

39
Q

what is an example of a covalent compound

A

methane - methane is a covalent compound

40
Q

what do ball and stick models show

A

ball ans stick models give an idea of the 3D shape of a molceule or compound

41
Q

what are some limitations of models of bonding

A

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
Q

what are simple molecules

A

simple molecules are when non metals or non ionic molecules join together, the atoms share electrons are form a covalent bond

43
Q

what is an example of a covalent molecule

A

hydrogen gas

44
Q

when are giant covalent structures formed

A

giant covalent structures are formed when the atoms of a substance form repeated covalent bonds. an exmaple is silicon dioxide

45
Q

when is a polymer formed

A

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
Q

how are metal atoms held together

A

metal atoms are held together by strong metallic bonds

47
Q

how do metals become positively charged

A

the metals become positively charged when the metal atoms lose their outermost electrons

48
Q

how is a sea of delocalised (free) electrons formed

A

a sea of delocalised (free) electrons is formed because electrons can move freely from one metal ion to another

49
Q

what does an element contain

A

an element contains one type of atom

50
Q

what cannot be chemically broken down into simpler substances

A

elements cannot be chemically broken down into simpler substances

51
Q

how many naturally occuring elements are there

A

there are about 100 naturally occurring elements

52
Q

who developed the design of the modern periodic table

A

the design of the modern period table was first developed by Mendeleev

53
Q

In Mendeleev’s table, what were the elements (placed into groups) based off of

A

In Mendeleev’s table, the elements were placed into groups based on their atomic mass w

54
Q

In Mendeleev’s table, why were some elements put into the wrong places

A

some elements were put into the wrong places because the values used for their atomic mass were incorrect

55
Q

what does the modern periodic table take into account

A

the modern periodic table takes into account the arrangement of electrons, the number of electrons in the outermost shell, and atomic number

56
Q

what is a group, in the periodic table

A

a group is a vertical column of elements

57
Q

what is a period, in the periodic table

A

a period is a horizontal row of elements

GCSE Chemistry (12 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions