periodic table of elements task 1a (1)
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8/4/2019 Periodic Table of Elements Task 1a (1)
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1 Task 1a – Unit 1 Fundamentals in Science (BTEC National Diploma in Applied Sciences)
Otgon Orgil
Periodic Table of Elements
Many of the elements (in compounds and their solutions) involved in carrying out the
preparation of standard solutions and titrations are in different groups and periods of
the periodic table.Using the elements sodium, potassium, calcium, magnesium, carbon, oxygen,
nitrogen, fluorine, chlorine, iron, hydrogen and sulphur, provide some key features of
the periodic table such as:
Their atomic number and relative atomic masses
Their electronic structures
How they are organised in groups, periods and blocks.
Any trends in their chemical properties (chemical reactivity down group I with
water & displacement reactions down group VII). Use balance chemical
equations to explain the trend down group I and VIII
Any trends in physical properties (Ionisation Energy & atomic radii) down a
group and across a period
Atomic number: 11
Relative Atomic Mass: 22.98976928 (2)
Group in periodic table: 1
Group name: Alkali metal
Period in periodic table: 3
Block in periodic table: s-block
Ionization energy (eV): 5.1391
Calculated Atomic Radii: 190
Electronic configurations: 2,8,1 or [Ne] 3s1
Atomic number: 19
Relative Atomic Mass: 39.0983 (1)
Group in periodic table: 1
Group name: Alkali metal
Period in periodic table: 4
Block in periodic table: s-block
Ionization energy (eV): 4.3407
Calculated Atomic Radii: 243
Electronic configurations: 2,8,8,1 or [Ar] 4s1
Atomic number: 20
Relative Atomic Mass: 40.078 (4)
Group in periodic table: 2
Group name: Alkali metal
Period in periodic table: 4
Block in periodic table: s-block
Ionization energy (eV): 6.1132
Calculated Atomic Radii: 194
Electronic configurations: 2,8,8,2 or [Ar] 4s2
11
Na Sodium
22.99
19
K Potassium
39.10
20
Ca Calcium
40.08
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2 Task 1a – Unit 1 Fundamentals in Science (BTEC National Diploma in Applied Sciences)
Otgon Orgil
Atomic number: 12
Relative Atomic Mass: 24.3050 (6)
Group in periodic table: 2
Group name: Alkaline earth metal
Period in periodic table: 3
Block in periodic table: s-block
Ionization energy (eV): 7.6462
Calculated Atomic Radii: 145
Electronic configurations: 2,8,2 or [Ne] 3s2
Atomic number: 6Relative Atomic Mass: 12.0107 (8)
Group in periodic table: 14
Group name: NA
Period in periodic table: 2
Block in periodic table: p-block
Ionization energy (eV): 11.2603
Calculated Atomic Radii: 67
Electronic configurations: 2,4 or [He] 2s2 2p2
Atomic number: 8
Relative Atomic Mass: 15.9994 (3)
Group in periodic table: 16
Group name: Chalcogen
Period in periodic table: 2
Block in periodic table: p-block
Ionization energy (eV): 13.6181
Calculated Atomic Radii: 48
Electronic configurations: 2,6 or [He] 2s2 2p4
Atomic number: 7
Relative Atomic Mass: 14.0067 (2)
Group in periodic table: 15
Group name: Pnictogen
Period in periodic table: 2
Block in periodic table: p-block
Ionization energy (eV): 14.5341
Calculated Atomic Radii: 56
Electronic configurations: 2,5 or [He] 2s2 2p3
12
Mg Magnesium
24.31
6
C Carbon
12.01
8
O Oxygen
16.00
7
N Nitrogen
14.01
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3 Task 1a – Unit 1 Fundamentals in Science (BTEC National Diploma in Applied Sciences)
Otgon Orgil
Atomic number: 9
Relative Atomic Mass: 18.9984032 (5)
Group in periodic table: 17
Group name: Halogen
Period in periodic table: 2
Block in periodic table: p-block
Ionization energy (eV): 17.4228
Calculated Atomic Radii: 42
Electronic configurations: 2,7 or [He] 2s2 2p5
Atomic number: 17
Relative Atomic Mass: 35.453 (2)Group in periodic table: 17
Group name: Halogen
Period in periodic table: 3
Block in periodic table: p-block
Ionization energy (eV): 12.9676
Calculated Atomic Radii: 79
Electronic configurations: 2,8,7 or [Ne] 3s2 3p5
Atomic number: 26
Relative Atomic Mass: 55.845 (2)
Group in periodic table: 8
Group name: NA
Period in periodic table: 4
Block in periodic table: -block
Ionization energy (eV): 7.9024
Calculated Atomic Radii: 156
Electronic configurations: 2,8,14,2 or [He] 3d6 4s2
Atomic number: 1Relative Atomic Mass: 1.00794 (7)
Group in periodic table: 1
Group name: NA
Period in periodic table: 1
Block in periodic table: s-block
Ionization energy (eV): 13.5984
Calculated Atomic Radii: 53
Electronic configurations: 2,7 or 1s1
9
F Fluorine
19.00
17
Cl Chlorine
35.45
26
Fe Iron
55.85
1
H Hydrogen
1.01
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4 Task 1a – Unit 1 Fundamentals in Science (BTEC National Diploma in Applied Sciences)
Otgon Orgil
Atomic number: 16
Relative Atomic Mass: 32.065 (5)
Group in periodic table: 16
Group name: ChalcogenPeriod in periodic table: 3
Block in periodic table: p-block
Ionization energy (eV): 10.36
Calculated Atomic Radii: 79
Electronic configurations: 2,8,6 or 3s2 3p4
Trends in chemical properties
I have observed seven (7) of the elements of the above are in the reactivity series of
metals. K, Na and Ca react with water in displacement. Mg, Fe and C react with
acids.
Going from bottom to top, the metals:
increase in reactivity;
lose electrons more readily to form positive ions; corrode or tarnish more readily;
require more energy (and different methods) to be separated from their ores;
become stronger reducing agents.
I have also observed group VII (Halogens) have water and displacement reactions.
The halogens become less reactive down the group. So bromine is less reactive thanchlorine, and iodine is less reactive than bromine. A more reactive halogen will
displace a less reactive halogen from an aqueous solution of its ions. Moreover, the
boiling points of the elements increase, elements become darker and less reactive
as oxidising agents when going down the group. They will also react with Group I to
form salts.
16
S Sulfur
32.07
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5 Task 1a – Unit 1 Fundamentals in Science (BTEC National Diploma in Applied Sciences)
Otgon Orgil
Definitions
Atomic mass (ma) is the total mass of protons, neutrons and electrons in a singleatom. There are three types of atomic masses: relative atomic mass, standard
atomic weight and relative isotopic mass. In this assignment, I will be predominately
using relative atomic mass primarily found in the periodic table. The relative atomic
mass is closest to the average atomic mass found in a particular sample, weighted
by isotopic abundance.
Atomic number (also known as the proton number) is the amount of protons found in
the nucleus of an atom, identical to the charge number of the nucleus. It is
conventionally represented as Z. The atomic number uniquely identifies a chemical
element.
A period is elements that are arrange in a series of rows so that those with similar
properties appear in a vertical column. Elements of the same period have the same
number of electron shells; with each group across a period, the elements have one
more proton and electron and become less metallic. This arrangement reflects the
periodic recurrence of similar properties as the atomic number increases. For
example, the alkaline metals lie in one group (group 1) and share similar properties,
such as high reactivity and the tendency to lose one electron to arrive at a noble-
gas electronic configuration.
A block in a periodic table is a set of adjacent groups. Each block is named after its
characteristic orbital.
There are 4 primary blocks and 1 hypothetical:
• s-block (alkali meals & alkaline earth metals - groups 1-2, periods 1-7)
• p-block (nonmetals & semimetals as well as some metals groups 13-18, periods 2-7)
• d-block (transition metals - groups 3-12, periods 4-7)
• f-block (inner transition metals – Lanthanoids plus Actinoids)
The following is the order for filling the "subshell" orbitals which also gives the linear
order of the "blocks" (as atomic number increases) in the periodic table: 1s, 2s, 2p, 3s,
3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p.
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6 Task 1a – Unit 1 Fundamentals in Science (BTEC National Diploma in Applied Sciences)
Otgon Orgil
A group in a periodic table is known as a family, a vertical column of chemical
elements. There are 18 groups in the periodic table. The modern explanation of thepattern of the table is that the elements in a group have similar configurations of the
outmost electron shells of the atoms (stabilization and destabilization, the same as
the core charge).
New IUPAC numbering Name
Group 1 the alkali metals or lithium family
Group 2 the alkaline earth metals or beryllium family
Group 3 the scandium family
Group 4 the titanium family
Group 5 the vanadium family
Group 6 the chromium family
Group 7 the manganese family
Group 8 the iron family
Group 9 the cobalt family
Group 10 the nickel family
Group 11 the copper family
Group 12 the zinc familyGroup 13 the boron group or boron family
Group 14 the carbon group or carbon family
Group 15 the pnictogens or nitrogen family
Group 16 the chalcogens or oxygen family
Group 17 the halogens or fluorine family
Group 18 the noble gases or helium family or neon family
Atomic radius is a term used to describe the
size of the atom, but there is no standard
definition for this value. Atomic radius may
refer to the ionic radius, covalent radius,metallic radius, or van der Waals radius. In all
cases, the size of the atom is dependent on
how far out the electrons exte nd. The
atomic radius for an element tends to
increase as one goes down an elementgroup. The electrons become more tightly
packed as you move across the periodic
table, so while there are more electrons for
elements of increasing atomic number, the atomic radius actually may decrease.
Group IAElements
ElectronicConfigurations
Numberof Shells
Group IIAElements
ElectronicConfigurations
Numberof Shells
Hydrogen 1 1 Beryllium 2,2 2
Lithium 2,1 2 Magnesium 2,8,2 3
Sodium 2,8,1 3 Calcium 2,8,8,2 4
Potassium 2,8,8,1 4 Strontium 2,8,18,8,2 5
Rubidium 2,8,18,8,1 5 Barium 2,8,18,18,8,2 6
Cesium 2,8,18,18,8,1 6 Radium 2,8,18,32,18,8,2 7
Francium 2,8,18,32,18,8,1 7
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7 Task 1a – Unit 1 Fundamentals in Science (BTEC National Diploma in Applied Sciences)
Otgon Orgil
Ionization energy is the amount of energy required to remove the highest-energy
electron from an isolated neutral atom in the gaseous state. Ionization Energy haspositive values because energy is always required to remove an electron, it is
endothermic. Electrons are attracted to the nucleus therefore energy is needed to
remove them.
Ionization Energy increases when: there is stronger nuclear charge - there is a full
subshell (therefore the atom is stable) - there is a half full subshell therefore there is
evenly distributed charge in the atom.
Ionization Energy is low when: there is more shielding - the electron to be removed is
spin paired (therefore there is repulsion) - the electron is far from the nucleus - when
an electron is in the next subshell, Ionization Energy will lower because the outer
electron is at a greater distance from the nucleus and there is more shielding from
inner subshells - when there is a half full subshell in an atom, the first Ionization Energy
is high because the atom is stable.
Tips
For any element:
Number of Protons = Atomic Number
Number of Electrons = Number of Protons = Atomic Number
Number of Neutrons = Mass Number - Atomic Number
Remember PEN