chem 2010_3 periodic trends
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PeriodicTrends
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Periodic Trends
Moving across the Periodic Table from leftto right, the elements
chemical and physical properties change from those of metalsto those
of metalloids(or semi-metals) and finally to those of non-metals:
Metals Metalloids Non-metals
Magnesium Silicon Sulphur
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Question:What are the typical chemical and physical properties of metals?
Good conductors of heat and electricity.
Tend to have high melting points and boiling points.
Tend to be hard and strong.
Tend to have a high density.
Have a metallic lustre (are shiny).
Malleable and ductile (shape can be changed without breaking). Sonorous (ring when struck).
React by losing their valence electrons.
Oxides are basic.
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Question:What are the typical chemical and physical properties of
non-metals?
Poor conductors of heat and electricity (insulators).
Tend to have low melting points and boiling points.
Tend to be soft.
Tend to have a low density.
Surface is dull (unless crystalline). Tend to be brittle.
Not sonorous.
React by gaining valence electrons.
Oxides are acidic.
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Question:
What are the typical chemical and physical properties of
metalloids?
Semiconductors (electrical conductivity varies greatly dependingupon the conditions that they are subject to).
Oxides are amphoteric (oxides can be either acidic or basicdepending upon the conditions that they are subject to).
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1 2 Group 3 4 5 6 7 0
1 H He
2 Li Be B C N O F Ne
3 Na Mg Al Si P S Cl Ar
4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
5Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
7 Fr Ra Ac
Period
Periodic Trends
The dividing linebetween metals (left)and non-metals (right).
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1 2 Group 3 4 5 6 7 0
1 H He
2 Li Be B C N O F Ne
3 Na Mg Al Si P S Cl Ar
4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
5Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
7 Fr Ra Ac
Period
Periodic Trends Metals!
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1 2 Group 3 4 5 6 7 0
1 H He
2 Li Be B C N O F Ne
3 Na Mg Al Si P S Cl Ar
4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
5Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
7 Fr Ra Ac
Period
Periodic Trends Metalloids!
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1 2 Group 3 4 5 6 7 0
1 H He
2 Li Be B C N O F Ne
3 Na Mg Al Si P S Cl Ar
4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
5Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
7 Fr Ra Ac
Period
Periodic Trends Non-metals!
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1 2 Group 3 4 5 6 7 0
1 H He
2 Li Be B C N O F Ne
3 Na Mg Al Si P S Cl Ar
4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
7 Fr Ra Ac
Period
Periodic Trends Summary!
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Periodic Trends
Question:
Lithium and sodium are both elements from Group 1 of the Periodic
Table.
Draw the electron configurations of lithium (atomic number = 3) andsodium (atomic number = 11):
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Periodic Trends
Question:
What do the electron configurations of the Group 1 metals have in
common?
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Answer:
The Group 1 metals all have 1 electron in their valence shell.
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Question:How do the Group 1 metals react to obtain a complete valence
shell?
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Answer:The Group 1 metals all react by losing their single valence electron to
form an ion with a complete valence shell and a single positive
charge. Because the Group 1 metals all react in this way, they are
said to have similar chemical properties.
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Question:Sodium (symbol Na) and caesium (symbol Cs) are both in
Group 1 of the Periodic Table.
The formula of sodium chloride is NaCl. The formula of sodium
carbonate is Na2CO3. The formula of sodium sulphate is Na2SO4.Using this information, predict the formulae of caesium chloride,
caesium carbonateand caesium sulphate.
Answer:Caesium chloride CsCl.
Caesium carbonate Cs2CO3.
Caesium sulphate Cs2SO4.
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Periodic Trends
Question:Some information about the Group 1 metals is given in the table
below:
Element Melting Point / C Metallic Radius / nm
Lithium Li 180.0 0.152
Sodium Na 97.8 0.186
Potassium K ? ?
Rubidium Rb 38.9 0.244
Caesium Cs 28.7 0.262
Predict the melting point and metallic radius of potassium.
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Periodic Trends
Answer:Some information about the Group 1 metals is given in the table
below:
Element Melting Point / C Metallic Radius / nm
Lithium Li 180.0 0.152
Sodium Na 97.8 0.186
Potassium K 63.7 0.231
Rubidium Rb 38.9 0.244
Caesium Cs 28.7 0.262
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Periodic Trends
Question:Fluorine and chlorine are both elements from Group 7 of the
Periodic Table.
Draw the electron configurations of fluorine (atomic number = 9)and chlorine (atomic number = 17):
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Periodic Trends
Question:What do the electron configurations of the Group 7 elements have
in common?
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Answer:The Group 7 elements all have 7 electrons in their valence shell.
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Question:How do the Group 7 elements react to obtain a complete valence
shell?
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Answer:The Group 7 elements all react by gaining a single valence electron to
form an ion with a complete valence shell and a single negative
charge. Because the Group 7 elements all react in this way, they are
said to have similar chemical properties.
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Periodic Trends
Question:Chlorine (symbol Cl) and astatine (symbol At) are both in
Group 7 of the Periodic Table.
The formula of sodium chloride is NaCl. The formula of magnesium
chloride is MgCl2. The formula of aluminium chloride isAlCl3. Usingthis information, predict the formulae of sodium astatide,
magnesium astatideand aluminium astatide.
Answer:Sodium astatide NaAt.
Magnesium astatide MgAt2.
Aluminium astatideAlAt3.
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Periodic Trends
Question:Some information about the Group 7 elements is given in the table
below:
Element Melting Point / C Covalent Radius / nm
Fluorine F 220 0.072
Chlorine Cl ? ?
Bromine Br 7.2 0.114
Iodine I 114 0.133
Astatine At 302 0.140
Predict the melting point and covalent radius of chlorine.
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Periodic Trends
Answer:Some information about the Group 7 elements is given in the table
below:
Element Melting Point / C Covalent Radius / nm
Fluorine F 220 0.072
Chlorine Cl 101 0.099
Bromine Br 7.2 0.114
Iodine I 114 0.133
Astatine At 302 0.140
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Periodic Trends
Question:Elements in the same Group of the Periodic Table have similar
chemical properties because they lose or gain the same number of
electrons to fill their valence shells. In what way do the elements in
the same Group of the Periodic Table differfrom each other?
Answer:The reactivityof the elements in the same Group varies. On
descending a Group of metals, the elements become more reactive.
On descending a Group of non-metals, the elements become less
reactive. In addition, the physical propertiesof the elements in the
same Group varies. On descending a Group of metals, their melting
points tends to decrease. On descending a Group of non-metals,
their melting points tends to increase.
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Periodic Trends
Question:Sodium and chlorine are both in the same Period of the
Periodic Table. Draw the electron configurations of sodium
(atomic number = 11) and chlorine (atomic number = 17) and
state in what way their electron configurations are similar to
each other.
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Answer:Sodium and chlorine are both in the thirdPeriod of the Periodic Table
and so both atoms have threeelectron shells:
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Question:Complete the table below to show how the properties of the elements
changes across the Periodic Table:
Group 1 2 3 4 5 6 7 0
Element Na Mg Al Si P S Cl Ar
Metal / Non-metal
Number of
Valence
Electrons
Number of
Electrons Lost /
Gained
Charge on Ion
Valency
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Question:Complete the table below to show how the properties of the elements
changes across the Periodic Table:
Group 1 2 3 4 5 6 7 0
Element Na Mg Al Si P S Cl Ar
Metal / Non-metal Metal Metal MetalSemi-
metal
Non-
metal
Non-
metal
Non-
metal
Non-
metal
Number of
Valence
Electrons
1 2 3 4 5 6 7 8
Number of
Electrons Lost /
Gained
1 Lost 2 Lost 3 Lost4
Gained
3
Gained
2
Gained
1
Gained
0 Lost
or
Gained
Charge on Ion +1 +2 +3 4 3 2 1 0
Valency 1 2 3 4 3 2 1 0
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Summary: Moving across the Periodic Table from leftto right, the elements
chemical and physical properties change from those of metalsto
those of metalloidsand finally to those of non-metals.
Elements in the same Grouphave the same number of valenceelectrons and therefore have similarchemical properties.
Elements from the same Groupform compounds with the same
formulae.
On descendinga Group of elements, there is a gradual change in
their chemical and physical properties. Metalsbecome morereactiveand their melting points decrease. Non-metalsbecome less
reactiveand their melting points increase.
Elements in the same Periodhave the same number of electron
shells.
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Enrichment:
Consider the elements of the third Period, sodium to chlorine.
How does the size (atomic radius) of an atom vary from leftto right across the Periodic Table?
How does the ease with which an atom loses an electronfrom its valence shell (first ionization energy) vary from left toright across the Periodic Table?
Clueconsider how atomic number changer across thePeriodic Table from sodium to chlorine. Remember what theatomic number of an element represents.
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Symbolof
Element
Na Mg Al Si P S Cl
Atomic
Number11 12 13 14 15 16 17
Atomic
Radius /
nm
0.157 0.136 0.125 0.117 0.110 0.104 0.099
First
Ionization
Energy /
kJ mol-1
494 736 577 786 1060 1000 1260
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Symbolof
Element
Na Mg Al Si P S Cl
Atomic
Number
Number of protons within the nucleus of the atom increases.
Positive charge within the nucleus of the atom increases.
Force of attraction between the positive nucleus and negative electrons orbitingthe nucleus increases.
Atomic
Radius /
nm
0.157 0.136 0.125 0.117 0.110 0.104 0.099
First
Ionization
Energy /
kJ mol-1
494 736 577 786 1060 1000 1260
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As the force of attraction between the positive nucleus and
negative electrons that are orbiting the nucleus increases, the
electrons are pulled in closer to the nucleus and the size of
the atom (atomic radius) decreases.
As the force of attraction between the positive nucleus and
negative electrons that are orbiting the nucleus increases, theamount of energy required to remove an electron from the
valence shell of an atom (first ionization energy) increases.
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A Note on First Ionization Energy
The ease with which an atom of a particular elementloses a single electron from its valence shell is given byits first ionization energy. This is the energy required to
convert one mole of gaseous atoms to one mole ofgaseous ions, each with a single positive charge. It canbe summarised by the following equation:
E(g)
E+(g)
+ e