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Chemistry > 1b:the periodic table > Flashcards

1b:the periodic table Flashcards

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1
Q

how were elements classified in the early periodic table?

A

atomic weight

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2
Q

why weren’t the elements classified by atomic number in the early periodic table?

A

scientists didn’t know about the atomic structure of protons,neutrons and electrons

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3
Q

what was the downfall of ordering the periodic table by atomic weight?

A

some elements were placed in columns with elements with dissimilar properties and their were gaps because of undiscovered elements.

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4
Q

why did Mendeleev leave gaps in his periodic table?

A

to make sure elements with similar properties stayed in the same groups and for elements he thought hadn’t been discovered and allowed Mendeleev to predict their properties.

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5
Q

How was Mendeleev proven right for leaving gaps?

A

When These elements were found and their properties fit Mendeleev’s predictions.eg.ekasilicon(now known as germanium)

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6
Q

how did the discovery of isotopes confirm that Mendeleev was correct to take into account the properties of elements when ordering them?

A

isotopes of the same element have different masses but the same chemical properties so they occupy the same place on the periodic table

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7
Q

how did Mendeleev order the elements in his periodic table?

A

mainly in order of atomic weight but he did switch the order of some elements if it meant that elements with similar properties could be placed in the same group

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8
Q

what is the periodic table?

A

a table containing all known elements named because similar properties occur at regular intervals.

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9
Q

what does the number of a group tell us about the element’s electronic structure?

A

all elements in the same group have the same number of electrons in their outer shell and therefore,similar chemical properties.

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10
Q

what are metals?

A

elements which can form positive ions when they react

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11
Q

what are non-metals?

A

elements which don’t form positive ions when they react and instead form negative ions in ionic compounds or bond covalently with other non-metals

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12
Q

why do atoms react?

A

they generally react to form full outer shells.

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13
Q

how do atoms react to form full outer shells?

A

either losing,gaining or sharing electrons.

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14
Q

why do metals lose electrons to get full outer shells?

A

metals to the left don’t have many electrons to lose and the outer electrons of the metals towards the bottom are further away from the nucleus so weaker attraction.Overall,less energy needed to lose electrons to form positive ions w/full outer shell

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15
Q

why do non metals gain or share electrons to get full outer shells?

A

towards the right of the periodic table,they have lots of electrons to remove to get a full outer shell and towards the top,the outer electrons are close to the nucleus so they have a strong attraction to it so its easier to share or gain electrons to get a full outer shell

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16
Q

what properties do metals commonly have?[3]

A

1.strong but malleable
2.great at conducting heat and electricity
3.generally have high b.p and m.p so normally solid at room temp

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17
Q

what properties do non-metals generally have?[4]

A

1.dull looking and more brittle
2.generally lower b.p and m.p than metals so aren’t always solids
3.generally don’t conduct electricity
4.often have lower densities than metals

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18
Q

properties of alkali metals?[4]

A

1.silvery solids stored in oils because they’re very reactive and react with air
2.low density(first three less dense than water)
3.low m.p and b.p
4.soft

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19
Q

what is the reactivity trend down the alkali metals?

A

reactivity increases down the group.This is because G1 react by losing their one outer shell electron.

As you go down, the outer electron is further away from the nucleus

so less attraction between them and so the outer electron is more easily

so the atom loses an electron more easily

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20
Q

what is the m.p and b.p trend for alkali metals?

A

m.p and b.p decreases down the group

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21
Q

what is the density trend down alkali metals?

A

density increases down the group because the further down you go,the more atoms there are

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22
Q

what do compounds produced when alkali metals react with non-metals look like and do?

A

The compounds that are produced when alkali metals react with non-metals are usually white solids that dissolve to form colourless solutions in water

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23
Q

what is the general equation for a alkali metal and water reaction

A

alkali metal+water->metal hydroxide+Hydrogen

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24
Q

how do lithium,sodium and potassium react with water?

A

they float and move around ,fizz as hydrogen gas is produced and sometimes,the reaction gets hot enough to ignite the hydrogen

(Fizz,Float,Flame)

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25
Q

what do the metal hydroxides that are formed from the reaction between alkali metal and water do in water?

A

dissolves in water to give alkaline solutions.

26
Q

what is the general equation of a alkali metal and chlorine reaction?

A

alkali metal+chlorine->metal chloride

27
Q

sodium and water balanced symbol equation

A

2Na(s)+2H ₂O(l) ->2NaOH(aq)+H ₂(g)

28
Q

sodium and chlorine balanced symbol equation

A

2Na(s)+Cl ₂(g)->2NaCl(s)

29
Q

what is the balanced symbol equation of the reaction between lithium and oxygen?

A

4Li(s)+O ₂(g)->2Li ₂O(s)

30
Q

what can the reaction between lithium and oxygen produce

A

lithium oxide

31
Q

what can sodium and oxygen react to produce?

A

a mixture of sodium oxide and sodium peroxide

32
Q

what is the balanced symbol equation of the reaction of sodium and oxygen to form sodium peroxide?

A

2Na(s)+O ₂(s)->Na ₂O ₂(s)

33
Q

what can potassium and oxygen react to form?

A

a mixture of potassium peroxide and potassium superoxide

34
Q

what is the balanced symbol equation of potassium and oxygen to form potassium superoxide?

A

K(s)+O ₂->KO ₂(s)

35
Q

how is the periodic table arranged?

A

increasing atomic number

36
Q

how many electrons do group 1 element atoms have in their outer shell?

A

1

37
Q

how many electrons do group 2 element atoms have in their outer shell?

A

2

38
Q

why do halogens all have similar chemical properties properties?

A

they all have the same number of electrons in the outer shell(seven)

39
Q

what is the colour,form and toxicity of fluorine?

A

poisonous yellow gas

40
Q

what is the colour,form,toxicity and density of chlorine?

A

poisonous dense green gas

41
Q

what is the colour,form,toxicity and density of bromine?

A

dense poisonous red-brown liquid or orange vapour

42
Q

what is the colour,form,toxicity and density of iodine ?

A

poisonous dark grey crystalline solid or purple vapour

43
Q

what are halogens?

A

non-metals

44
Q

what molecular form do halogens exist as?

A

diatomic molecules

45
Q

what is the reactivity trend down the halogens?

A

reactivity decreases down the group. This is because G1 react by gaining one outer shell electron.

As you go down, the outer electrons is further away from the nucleus so less attraction between them and so theirs less attraction from the nucleus pulling electrons into the atom.

46
Q

what is the melting and boiling point trend down the halogens?

A

the m.p and b.p increase as you go down the group.

47
Q

what is the relative atomic mass trend of halogens?

A

the relative atomic mass increases as you go down the group.

48
Q

how do halogens react with non-metals?

A

they share electrons via covalent bonding to achieve a full outer shell.The compounds that form all have simple molecular structures.

49
Q

how do halogens react with metals?

A

its easy to gain an extra electron.When halogens gain an electron they form 1- ions (halide ions)

50
Q

halogens:displacement reactions

A

a more reactive halogen can displace a less reactive halogen from an aqueous solution of its salt.

eg. Chlorine(g) would displace the bromine in potassium bromide(aq) to produce bromine(aq) + potassium chloride(aq)

51
Q

why are noble gases unreactive?

A

they have a full outer shell of electrons(energetically stable)

52
Q

how reactive are noble gases?

A

they are more or less inert(don’t react with much)

53
Q

what is the b.p and m.p trends of noble gases?

A

increase as you move down the group

54
Q

what is the relative atomic mass of trend down the nobles gases?

A

increases as you go down

55
Q

why does the b.p increase as you go down the noble gases?

A

the atomic number increases down the group so the number of electrons increases which causes the intermolecular forces between the atoms to increase so more energy is needed to break them so the b.p increases.

56
Q

how can you predict the properties pf elements in groups?

A

the trend in properties within groups means you can use the information about some elements to predict the properties in other elements

57
Q

what are transition metals?

A

metals with similar properties which are different those of the elements in groups 1.

58
Q

what are the properties of transition metals?

A

1.good conductors of heat and electricity
2.dense,strong and shiny

59
Q

how are transition metals different to alkali metals?[3]

A

1.TM are less reactive eg.Na fizzes violently with water but Mn doesn’t react with water at room temperature

2.TM are denser,stronger and harder.eg.K is soft and floats on water but Ni is harder and sinks

3.TM have higher m.p.eg.Fe melts at 1538 degrees wheras K melts at 63 degrees

60
Q

transition metal ions

A

TM can form ions of different charges eg.Copper can form Cu+ or Cu2+

61
Q

transition metals compounds

A

form colourful compound.The colour is due to the TM ions they contain eg.copper(II) sulfate is blue

62
Q

Transition metals as catalysts

A

TM and their compounds are good catalysts eg.Nickel is the catalyst used to hydrogenate alkenes

Chemistry (11 decks)

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