composition

structure

Matter
properties
Matter Defined

2
• Matter is anything that has mass
and occupies space.
• Matter can be invisible.
– Air is matter, but it cannot be seen.
...
An apparently empty test tube is submerged, mouth
downward in water. Only a small volume of water
rises into the tube, whi...
Physical States of
Matter
5
6
7
Pure Substances and
Mixtures
8
Matter refers to all of the materials that
make up the universe.

9
Classification of matter: A pure substance is
always homogeneous in composition, whereas a
mixture always contains two or ...
Pure Substance
A particular kind of matter that has a fixed
composition and distinct properties.

Examples
ammonia, water,...
Elements

12
An element is a fundamental or
elementary substance that cannot be
broken down into simpler substances by
any means

13
• All known substances on Earth and
probably the universe are formed by
combinations of more than 100
elements.
• Each ele...
• Most substances can be decomposed
into two or more simpler substances.
– Water can be decomposed into hydrogen
and oxyge...
Distribution of
Elements
16
• Elements are not distributed equally
by nature.
– Oxygen is the most abundant element in
the human body (65%).
– Oxygen ...
Distribution
of the
common
elements in
nature.

18
3.3
Names of the
Elements
19
Sources of Element Names
GreekColor

• Iodine: from the Greek iodes meaning
violet.

• Fluorine: from the Latin fluere mea...
Compounds
21
A compound is a distinct substance that
contains two or more elements combined
in a definite proportion by weight.
Compoun...
There are two types of compounds:
molecular and ionic.

23
Molecules

24
A molecule is the smallest uncharged
individual unit of a compound formed by
the union of two or more atoms.

25
• A water molecule consists of two
hydrogen atoms and one oxygen atom.
• If it is subdivided the water molecule
will be de...
Ionic Compounds

27
An ion is a positively or negatively
charged atom or group of atoms.

28
A cation is a positively charged ion.

29
3.5
An anion is a negatively charged ion.

30
3.5
Ionic compounds are held together by
attractive forces between positively and
negatively charged ions.

31
Sodium Chloride
The ultimate particles of sodium chloride
are positively charged sodium ions and
negatively charged chlori...
Compounds can be classified as molecular or
ionic. Ionic compounds are held together by
attractive forces between their po...
Mixture
Matter containing 2 or more substances that
are present in variable amounts. Mixtures
are variable in composition....
Homogeneous Mixture (Solution)
A homogeneous mixture of 2 or more
substances. It has one phase.

Example
Sugar and water. ...
Heterogeneous Mixture
A heterogeneous mixture consists of 2 or
more phases.

Example
Sugar and fine white sand. The amount...
Heterogeneous Mixture
A heterogeneous mixture consists of 2 or more
phases.

Example

• Iron (II) sulfide (FeS) is 63.5% F...
Mixture of iron
and sulfur

Compound of iron
and sulfur

Formula

Has no definite
formula: consists
of Fe and S.

FeS

Com...
39
Symbols of the
Elements
40
• A symbol stands for
– the element itself
– one atom of the element
– a particular quantity of the element

41
Rules governing symbols of the elements
are:
1. Symbols have either one or
two letters.
2. If one letter is used it is
cap...
These symbols have carried over from the earlier names of the
A number of symbols Latin). to the sameconnection with the e...
44
Metals, Nonmetals
and Metalloids
45
Metals

46
Most elements
are metals

47
• Metals are solid at room temperature.
– Mercury is an exception. At room temperature it
is a liquid.
• Metals are good c...
• Metals are ductile (they can be drawn into wires).
• Most metals have a high melting point.

Most elements
are metals
• ...
Examples of Metals

lead
gold
iron
50
Chemical Properties of Metals
• Metals have little tendency to combine with
each other to form compounds.
• Many metals re...
Chemical Properties of Metals

– A few of the less reactive metals such as copper,
silver and gold are found in the free s...
Nonmetals

53
Physical Properties of Nonmetals
• Lack luster (they are dull)
• Have relatively low melting points
• Have low densities.
...
Physical State at Room Temperature

phosphorous

carbon

Solid
selenium

sulfur
iodine

55
Physical State at Room Temperature

liquid

bromine

56
Physical State at Room Temperature

nitrogen,
oxygen

gas

fluorine,
chlorine

helium, neon, argon, krypton, xenon, radon
...
Metalloids

58
Metalloids have properties that
are intermediate between metals
and nonmetals

59
The Metalloids
1. boron
2. silicon
3. germanium
4. arsenic
5. antimony
6. tellurium
7. polonium
60
Nonmetals found to to left of the the metalloids.
Metals are are found thethe right of metalloids

61
In 1869 Dimitri Mendeleev of Russia and
Lothar Meyer of Germany independently
published periodic arrangements of the
eleme...
Period numbers correspond
Horizontal rows are
to the highest occupied
called periods.
energy level.

63
10.14
Elements in the A groups
Elements in the B groups
with similar
Groups are numbered
are designated organized
properties are...
Period number corresponds with the
highest energy level occupied by
electrons in that period.
65
10.17
The group numbersfamily have the same
The elements of a for the representative
outermost electron configurationnumber that...
Noble Gas
Halogen

Group

Alkali Metal

Alkali Earth Metal

Period
Periodic Trends in
Atomic Properties
68
Characteristic properties and trends of the
elements are the basis of the periodic
table’s design.

69
These trends allow us to use the periodic
table to accurately predict properties and
reactions of a wide variety of substa...
Atomic Radius

71
Radii of atoms
increase down a
group.

For each step down a group, electrons enter
the next higher energy level.

72
11.2
Radii of atoms tend to decrease
from left to right across a period.
This
Each time an
For increase in
positive is added
el...
Radii of atoms tend to decrease
from left to right across a period.
Each
This time an
For increase in
electron is added
po...
Ionization Energy

75
The ionization energy of an atom is the
energy required to remove an electron from
an atom.
Na + ionization energy → Na+ +...
As each succeeding electron is removed from
an atom ever higher energies are required.

77
The Atom
Atom is the basic unit of an element,
made up of even smaller particles
called subatomic particles.
There are thr...
The Structure of the Atom
The Structure of the Atom

Electron (cloud)

Nucleus

Figure above shows the location of the pro...
Subatomic Particles

mass p = mass n = 1840 x mass e-
Atomic Numbers of
the Elements
81
Atomic Number, Mass Number & Isotopes

Atomic number (Z)

= number of protons in nucleus

Mass number (A)

= number of pro...
• The atomic number of an element is
equal to the number of protons in the
nucleus of that element.
• The atomic number of...
Every atom with an atomic
number of 1 is a hydrogen atom.
Every hydrogen atom contains 1
proton in its nucleus.

84
Every atom with an atomic
number of 6 is a carbon atom.
Every carbon atom contains 6
protons in its nucleus.

85
atomic
number
Every atom with an
atomic number of 1
is a hydrogen atom.
1 proton in the
nucleus

H
1

86
atomic
number
Every atom with an
atomic number of 6
is a carbon atom.
6 protons in the
nucleus

C
6

87
atomic
number

U
92

Every atom with an
atomic number of
92 is a uranium
atom.
92 protons
in the
nucleus

88
Isotopes of the
Elements
89
• Atoms of the same element can have
different masses.
• They always have the same number of
protons, but they can have di...
Isotopic Notation

91
Isotopic Notation
6 protons + 6 neutrons

12
C
6
6 protons

92
Isotopic Notation
6 protons + 8 neutrons

14
C
6
6 protons

93
Isotopic Notation
8 protons + 8 neutrons

16
O
8
8 protons

94
Isotopic Notation
8 protons + 9 neutrons

17
O
8
8 protons

95
Isotopic Notation
8 protons + 10 neutrons

18
O
8
8 protons

96
Hydrogen has three isotopes

1 proton

1 proton

1 proton

0 neutrons

1 neutron

2 neutrons
97
Relationship Between Mass
Number and Atomic Number
98
The mass number minus the atomic
number equals the number of neutrons in
the nucleus.
mass
number
atomic
number

atomic
ma...
Energy Levels
of Electrons
100
As n increases, the
energy of the electron
increases.
The first four
principal energy
levels of an atom.
Each level is
ass...
10.7, 10.8

Each principal energy level
is subdivided into sublevels.

102
Within sublevels the electrons are found in
orbitals.
An s orbital is spherical in
shape.
The
spherical
surface
encloses a...
An atomic orbital can hold a maximum of two
electrons.
An electron can spin in one
of two possible directions
represented ...
A p sublevel is made up of three orbitals.

Each p orbital has two lobes.
Each p orbital can hold a maximum of two
electro...
pz

The three p orbitals share
a common center.
py

px

The three p orbitals point
in different directions.

106
10.10
A d sublevel is made up of five orbitals.

The five d orbitals all point in different directions.
Each d orbital can hold ...
10.8 10.10 10.11

Number of Orbitals in a Sublevel

108
Distribution of Subshells by
Principal Energy Level
n=1

1s

n=2

2s

2p 2p 2p

n = 3 3s

3p 3p 3p

3d 3d 3d 3d 3d

n = 4 ...
Nuclear makeup and electronic structure of
each principal energy level of an atom.

number of protons and electrons
number...
Electron Configuration
Number of
electrons in
sublevel orbitals

Arrangement of
electrons within their
respective sublevel...
The electron configuration of any of the
noble gas elements can be represented by
the symbol of the element enclosed in
sq...
The electron configuration of argon is
Ar 1s22s22p63s23p6
The elements after argon are potassium
and calcium. Instead of e...
d orbital numbers are 1 less
than d orbital filling
the period number

10.16

Arrangement of electrons
according to sublev...
f orbital numbers are 2 less
than fthe period number
orbital filling

10.16

Arrangement of electrons
according to subleve...
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Classifying matter

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Lesson 2, Classifying matter- Solid, Liquid, Gas and the others

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Classifying matter

  1. 1. composition structure Matter properties
  2. 2. Matter Defined 2
  3. 3. • Matter is anything that has mass and occupies space. • Matter can be invisible. – Air is matter, but it cannot be seen. • Matter appears to be continuous and unbroken. – Matter is actually discontinuous. It is made up of tiny particles call atoms. 3
  4. 4. An apparently empty test tube is submerged, mouth downward in water. Only a small volume of water rises into the tube, which is actually filled with invisible matter–air. 4 3.1
  5. 5. Physical States of Matter 5
  6. 6. 6
  7. 7. 7
  8. 8. Pure Substances and Mixtures 8
  9. 9. Matter refers to all of the materials that make up the universe. 9
  10. 10. Classification of matter: A pure substance is always homogeneous in composition, whereas a mixture always contains two or more substances and may be either homogeneous or heterogeneous. 3.2 10
  11. 11. Pure Substance A particular kind of matter that has a fixed composition and distinct properties. Examples ammonia, water, and oxygen. 11
  12. 12. Elements 12
  13. 13. An element is a fundamental or elementary substance that cannot be broken down into simpler substances by any means 13
  14. 14. • All known substances on Earth and probably the universe are formed by combinations of more than 100 elements. • Each element has a number. – Beginning with hydrogen as 1 the elements are numbered in order of increasing complexity. 14
  15. 15. • Most substances can be decomposed into two or more simpler substances. – Water can be decomposed into hydrogen and oxygen. – Table salt can be decomposed into sodium and chlorine. • An element cannot be decomposed into a simpler substance. 15
  16. 16. Distribution of Elements 16
  17. 17. • Elements are not distributed equally by nature. – Oxygen is the most abundant element in the human body (65%). – Oxygen is the most abundant element in the crust of the earth (49.2%).. • In the universe the most abundant element is hydrogen (91%) and the second most abundant element is helium (8.75%). 17
  18. 18. Distribution of the common elements in nature. 18 3.3
  19. 19. Names of the Elements 19
  20. 20. Sources of Element Names GreekColor • Iodine: from the Greek iodes meaning violet. • Fluorine: from the Latin fluere meaning to LatinProperty flow. German- • Bismuth: from the German Color weisse mass which means white mass. Location • Germanium: discovered in 1866 by a German chemist. Famous- • Einsteinium: named for Albert Einstein. 20 Scientists
  21. 21. Compounds 21
  22. 22. A compound is a distinct substance that contains two or more elements combined in a definite proportion by weight. Compounds can be decomposed chemically into simpler substances–that is, into simpler compounds or elements. 22
  23. 23. There are two types of compounds: molecular and ionic. 23
  24. 24. Molecules 24
  25. 25. A molecule is the smallest uncharged individual unit of a compound formed by the union of two or more atoms. 25
  26. 26. • A water molecule consists of two hydrogen atoms and one oxygen atom. • If it is subdivided the water molecule will be destroyed and hydrogen and oxygen will be formed. 26 3.5
  27. 27. Ionic Compounds 27
  28. 28. An ion is a positively or negatively charged atom or group of atoms. 28
  29. 29. A cation is a positively charged ion. 29 3.5
  30. 30. An anion is a negatively charged ion. 30 3.5
  31. 31. Ionic compounds are held together by attractive forces between positively and negatively charged ions. 31
  32. 32. Sodium Chloride The ultimate particles of sodium chloride are positively charged sodium ions and negatively charged chloride ions. 32 3.5
  33. 33. Compounds can be classified as molecular or ionic. Ionic compounds are held together by attractive forces between their positive and negative charges. Molecular compounds are held together by covalent bonds. 33 3.4
  34. 34. Mixture Matter containing 2 or more substances that are present in variable amounts. Mixtures are variable in composition. They can be homogeneous or heterogeneous. 34
  35. 35. Homogeneous Mixture (Solution) A homogeneous mixture of 2 or more substances. It has one phase. Example Sugar and water. Before the sugar and water are mixed each is a separate phase. After mixing the sugar is evenly dispersed throughout the volume of the water. 35
  36. 36. Heterogeneous Mixture A heterogeneous mixture consists of 2 or more phases. Example Sugar and fine white sand. The amount of sugar relative to sand can be varied. The sugar and sand each retain their own properties. 36
  37. 37. Heterogeneous Mixture A heterogeneous mixture consists of 2 or more phases. Example • Iron (II) sulfide (FeS) is 63.5% Fe and 36.5% S by mass. • Mixing iron and sulfur in these proportions does not form iron (II) sulfide. Two phases are present: a sulfur phase and an iron phase. • If the mixture is heated strongly a chemical reaction occurs and iron (II) sulfide is formed. • FeS is a compound of iron and sulfur and has 37 none of the properties of iron and sulfur.
  38. 38. Mixture of iron and sulfur Compound of iron and sulfur Formula Has no definite formula: consists of Fe and S. FeS Composition Contains Fe and S in any proportion by mass. 63.5% Fe and 36.5% S by mass. Separation Fe and S can be separated by physical means. Fe and S can be separated only by chemical change. 38
  39. 39. 39
  40. 40. Symbols of the Elements 40
  41. 41. • A symbol stands for – the element itself – one atom of the element – a particular quantity of the element 41
  42. 42. Rules governing symbols of the elements are: 1. Symbols have either one or two letters. 2. If one letter is used it is capitalized. C hydrogen H carbon 3. If two letters are used, only Ne barium Ba neon the first is capitalized. 42
  43. 43. These symbols have carried over from the earlier names of the A number of symbols Latin). to the sameconnection with the element. elements (usually start with have no letter as the element. Most symbols appear 43
  44. 44. 44
  45. 45. Metals, Nonmetals and Metalloids 45
  46. 46. Metals 46
  47. 47. Most elements are metals 47
  48. 48. • Metals are solid at room temperature. – Mercury is an exception. At room temperature it is a liquid. • Metals are good conductors of heat and electricity. Most elements are metals physical properties of or • Metals are malleable (they can be rolledmetals hammered into sheets). • Metals have high luster (they are shiny). 48
  49. 49. • Metals are ductile (they can be drawn into wires). • Most metals have a high melting point. Most elements are metals • Metals have high densities 49
  50. 50. Examples of Metals lead gold iron 50
  51. 51. Chemical Properties of Metals • Metals have little tendency to combine with each other to form compounds. • Many metals readily combine with nonmetals to form ionic compounds. – They can combine with sulfur. oxygen. chlorine. – In nature, minerals are formed by combinations of the more reactive metals combined with other elements. 51
  52. 52. Chemical Properties of Metals – A few of the less reactive metals such as copper, silver and gold are found in the free state. – Metals can mix with each other to form alloys.  Brass is a mixture of copper and zinc.  Bronze is a mixture of copper and tin.  Steel is a mixture of carbon and iron. 52
  53. 53. Nonmetals 53
  54. 54. Physical Properties of Nonmetals • Lack luster (they are dull) • Have relatively low melting points • Have low densities. • Poor conductors of heat and electricity • At room temperature carbon, phosphorous, sulfur, selenium, and iodine are solids. 54
  55. 55. Physical State at Room Temperature phosphorous carbon Solid selenium sulfur iodine 55
  56. 56. Physical State at Room Temperature liquid bromine 56
  57. 57. Physical State at Room Temperature nitrogen, oxygen gas fluorine, chlorine helium, neon, argon, krypton, xenon, radon 57
  58. 58. Metalloids 58
  59. 59. Metalloids have properties that are intermediate between metals and nonmetals 59
  60. 60. The Metalloids 1. boron 2. silicon 3. germanium 4. arsenic 5. antimony 6. tellurium 7. polonium 60
  61. 61. Nonmetals found to to left of the the metalloids. Metals are are found thethe right of metalloids 61
  62. 62. In 1869 Dimitri Mendeleev of Russia and Lothar Meyer of Germany independently published periodic arrangements of the elements based on increasing atomic masses. Mendeleev’s arrangement is the precursor to the modern periodic table. 62
  63. 63. Period numbers correspond Horizontal rows are to the highest occupied called periods. energy level. 63 10.14
  64. 64. Elements in the A groups Elements in the B groups with similar Groups are numbered are designated organized properties are transition are designated with Roman numerals. in groups or families. representative elements. elements. 64 10.14
  65. 65. Period number corresponds with the highest energy level occupied by electrons in that period. 65 10.17
  66. 66. The group numbersfamily have the same The elements of a for the representative outermost electron configurationnumber that elements are equal to the total except of outermost electrons in the atoms of the group. the electrons are in different energy levels. 66 10.17
  67. 67. Noble Gas Halogen Group Alkali Metal Alkali Earth Metal Period
  68. 68. Periodic Trends in Atomic Properties 68
  69. 69. Characteristic properties and trends of the elements are the basis of the periodic table’s design. 69
  70. 70. These trends allow us to use the periodic table to accurately predict properties and reactions of a wide variety of substances. 70
  71. 71. Atomic Radius 71
  72. 72. Radii of atoms increase down a group. For each step down a group, electrons enter the next higher energy level. 72 11.2
  73. 73. Radii of atoms tend to decrease from left to right across a period. This Each time an For increase in positive is added electron nuclear representative a charge pulls all proton is within elements a added to electrons closer the same period to nucleus. the energy level nucleus. remains constant as electrons are added. 73 11.2
  74. 74. Radii of atoms tend to decrease from left to right across a period. Each This time an For increase in electron is added positive nuclear representative a proton pulls all charge is within elements added to electrons closer the same period to nucleus. the energy level nucleus. remains constant as electrons are added. 74 11.2
  75. 75. Ionization Energy 75
  76. 76. The ionization energy of an atom is the energy required to remove an electron from an atom. Na + ionization energy → Na+ + e- 76
  77. 77. As each succeeding electron is removed from an atom ever higher energies are required. 77
  78. 78. The Atom Atom is the basic unit of an element, made up of even smaller particles called subatomic particles. There are three fundamental components (subatomic particles) that are important in chemistry: Electron, Proton and Neutron. The protons and neutrons of an atom are packed in an extremely small nucleus. Electrons are shown as ‘clouds’ around the nucleus.
  79. 79. The Structure of the Atom The Structure of the Atom Electron (cloud) Nucleus Figure above shows the location of the protons, Neutrons and electrons in an atom
  80. 80. Subatomic Particles mass p = mass n = 1840 x mass e-
  81. 81. Atomic Numbers of the Elements 81
  82. 82. Atomic Number, Mass Number & Isotopes Atomic number (Z) = number of protons in nucleus Mass number (A) = number of protons + number of neutrons = atomic number (Z) + number of neutrons Isotopes are atoms of the same element (X) with different numbers of neutrons in their nuclei Mass Number Atomic Number A ZX Element Symbol
  83. 83. • The atomic number of an element is equal to the number of protons in the nucleus of that element. • The atomic number of an atom determines which element the atom is. 83
  84. 84. Every atom with an atomic number of 1 is a hydrogen atom. Every hydrogen atom contains 1 proton in its nucleus. 84
  85. 85. Every atom with an atomic number of 6 is a carbon atom. Every carbon atom contains 6 protons in its nucleus. 85
  86. 86. atomic number Every atom with an atomic number of 1 is a hydrogen atom. 1 proton in the nucleus H 1 86
  87. 87. atomic number Every atom with an atomic number of 6 is a carbon atom. 6 protons in the nucleus C 6 87
  88. 88. atomic number U 92 Every atom with an atomic number of 92 is a uranium atom. 92 protons in the nucleus 88
  89. 89. Isotopes of the Elements 89
  90. 90. • Atoms of the same element can have different masses. • They always have the same number of protons, but they can have different numbers of neutrons in their nuclei. • The difference in the number of neutrons accounts for the difference in mass. • These are isotopes of the same element. 90
  91. 91. Isotopic Notation 91
  92. 92. Isotopic Notation 6 protons + 6 neutrons 12 C 6 6 protons 92
  93. 93. Isotopic Notation 6 protons + 8 neutrons 14 C 6 6 protons 93
  94. 94. Isotopic Notation 8 protons + 8 neutrons 16 O 8 8 protons 94
  95. 95. Isotopic Notation 8 protons + 9 neutrons 17 O 8 8 protons 95
  96. 96. Isotopic Notation 8 protons + 10 neutrons 18 O 8 8 protons 96
  97. 97. Hydrogen has three isotopes 1 proton 1 proton 1 proton 0 neutrons 1 neutron 2 neutrons 97
  98. 98. Relationship Between Mass Number and Atomic Number 98
  99. 99. The mass number minus the atomic number equals the number of neutrons in the nucleus. mass number atomic number atomic mass number number 109 47 = = number of neutrons 62 99
  100. 100. Energy Levels of Electrons 100
  101. 101. As n increases, the energy of the electron increases. The first four principal energy levels of an atom. Each level is assigned a principal quantum number n. 101 10.7
  102. 102. 10.7, 10.8 Each principal energy level is subdivided into sublevels. 102
  103. 103. Within sublevels the electrons are found in orbitals. An s orbital is spherical in shape. The spherical surface encloses a space where there is a 90% probability that the electron may be found. 103 10.10
  104. 104. An atomic orbital can hold a maximum of two electrons. An electron can spin in one of two possible directions represented by ↑ or ↓. The two electrons that occupy an atomic orbital must have opposite spins. This is known as the Pauli Exclusion Principal. 104 10.10
  105. 105. A p sublevel is made up of three orbitals. Each p orbital has two lobes. Each p orbital can hold a maximum of two electrons. A p sublevel can hold a maximum of 6 electrons. 10.10 105
  106. 106. pz The three p orbitals share a common center. py px The three p orbitals point in different directions. 106 10.10
  107. 107. A d sublevel is made up of five orbitals. The five d orbitals all point in different directions. Each d orbital can hold a maximum of two electrons. A d sublevel can hold a maximum of 10 electrons. 10.11 107
  108. 108. 10.8 10.10 10.11 Number of Orbitals in a Sublevel 108
  109. 109. Distribution of Subshells by Principal Energy Level n=1 1s n=2 2s 2p 2p 2p n = 3 3s 3p 3p 3p 3d 3d 3d 3d 3d n = 4 4s 4p 4p 4p 4d 4d 4d 4d 4d 4f 4f 4f 4f 4f 4f 4f 109
  110. 110. Nuclear makeup and electronic structure of each principal energy level of an atom. number of protons and electrons number of neutrons in thein each sublevel nucleus 110 10.13
  111. 111. Electron Configuration Number of electrons in sublevel orbitals Arrangement of electrons within their respective sublevels. 2p 6 Principal Type of orbital energy level 111
  112. 112. The electron configuration of any of the noble gas elements can be represented by the symbol of the element enclosed in square brackets. B 1s22s22p1 [He]2s22p1 Na 1s22s22p63s1 [Ne]3s1 Cl 1s22s22p63s23p5 [Ne]3s23p5 112
  113. 113. The electron configuration of argon is Ar 1s22s22p63s23p6 The elements after argon are potassium and calcium. Instead of entering a 3d orbital, the valence electrons of these elements enter the 4s orbital. K 1s22s22p63s23p64s1 [Ar]4s1 Ca 1s22s22p63s23p6 4s2 [Ar]4s2 113
  114. 114. d orbital numbers are 1 less than d orbital filling the period number 10.16 Arrangement of electrons according to sublevel being filled. 114
  115. 115. f orbital numbers are 2 less than fthe period number orbital filling 10.16 Arrangement of electrons according to sublevel being filled. 115

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