9. 2.
A type of bond that exists when two
bonded atoms are not equally
bonded, one atom is partially
positive and the other is partially
negative.
10. 2. Polar bond
A type of bond that exists when two
bonded atoms are not equally
bonded, one atom is partially
positive and the other is partially
negative.
11. 3.
A bond formed between
two identical atoms with
relatively close
electronegativity values.
17. 1
Differentiate polar molecule
from non-polar molecule
2
Determine whether the bond
between atoms is polar,
nonpolar, or ionic based on
electronegativity difference
18. What do you
remember?
•Ionic and Covalent Compounds
•Electronic Configuration
•Valence Electron and Lewis Dot
Symbol
19.
20.
21. •Ionic bonds form when two oppositely
charged atoms (called ions) transfer their
electrons (negatively charged particles) to create
a secure bond between the two.Most often, you’ll
see this bond happen between a metal and
nonmetal.
•Covalent bonds are created when atoms
share their electrons. Covalent bonds happen
between two nonmetals.
• Metallic bonds.Metal shares electrons with
another metal.
3 Types of Chemical Bonding
32. 2. A chemical bond formation that involves the
complete transfer of electrons between atoms is
_______
A. Ionic bond
B. Covalent bond
C. Metallic bond
D. Partial covalent bond
33. 3. Covalent bonds are created when atoms share
their electrons. Covalent bonds happen between
__________.
A.2 Metals
B.2 Non metals
C.Metals and Non metals
34. 4. Two oppositely charged ions are positive ions
known as ________ and negative ions known as
_________.
A.Cation & Anion
B.Anion & Cation
37. Electronic Configuration
• refers to the arrangement of the electron within the orbitals of an atom to
know more about an atom’s electronic property.
39. • Chlorine has an atomic number of 17.
• The electron configuration of chlorine is illustrated below. It can
be written as 1s2 2s2 2p6 3s2 3p5
Chlorine Electronic Configuration
40. •Determining the valency of an element.
•Predicting the properties of a group of
elements (elements with similar electron
configurations tend to exhibit similar
properties).
Electronic Configuration are
useful for:
41.
42. • Valence electrons are the electrons
located at the outermost shell of an
atom, involved in chemical bonding.
• Octet Rule states that atoms tend to
form compounds in ways that give
them 8 valence electrons and thus the
electronic configuration of noble gas
•Lewis Dot Symbol/Structures are
diagrams that represent the valence
diagram of an atom
43.
44.
45. Valence Electron & Lewis Dot Symbol
• Sodium Chloride
11Na 1s2 2s2 2p6 3s1
17Cl 1s2 2s2 2p6 3s2 3p5
46. How do you find the valence
electrons?
• For neutral atoms, the number of valence electrons is equal to
the atom’s main group number. The main group number for an
element can be found from its column on the periodic table.
• For example, carbon is in group 4 and has 4 valence electrons.
• Oxygen is in group 6 and has 6 valence electrons.
52. 1. Which element has an electronic
configuration of 1s2 2s2 2p5 ?
A. Carbon
B. Oxygen
C. Fluorine
D. Hydrogen
53. 2. Which of the orbitals has the highest
energy?
A. 1s
B. 2s
C. 2p
D. 3s
54. 3. Which element has an electronic
configuration of 1s2 2s2 2p6 3s2 3p1 ?
A. Aluminum
B. Neon
C. Silicon
D. Sodium
55. 4. Can orbital 3f exist?
A. Yes
B. No
C. Maybe
D. Not sure
56. 5.Electrons in the outer shells that are not
filled are called
A. Valence electrons
B. Shell electrons
C. Last electrons
D. All of these
57. 6.How many valence electrons does
Sulfur have?
A. Eight
B. Seven
C. Six
D. Five
58. 7.Among the noble gases which does
not have 8 valence electrons in its
outermost shell?
A. Ne
B. Xe
C. He
D. Ar
59. 8.What is the valence electron
of Halogens ?
A. 8
B. 7
C. 6
D. 5
60. 9. Atoms with unpaired electrons are
___________.
A. Lone pair
B. Single atoms
C. Fake atoms
D. Paramagnetic
61. 10. What distribution does the electronic
configration describe?
A. Protons
B. Neutrons
C. Electrons
D. Ions
62. 11. Which is the first noble gas?
A. Helium
B. Xenon
C. Krypton
D. Radon
63.
64. • A bond formed between two identical atoms with relatively close
electronegativity values.
• Covalent bonds are created when atoms share their electrons.
Covalent bonds happen between two nonmetals.
• Can be classified into two: non-polar covalent bond and polar
covalent bond.
Covalent Bond
65. • Polarity, in general, refers to the physical properties of compounds such as
boiling point, melting points, and their solubilities.
• Polarity is used in areas like magnetism, electricity, and signalling of
electronic devices. Consider an electromotive force (EMF) or an electric
potential, acting between two points. Here the points or poles as they are
commonly known as have more electrons than the other. The pole having
more electrons possesses a negative polarity whereas the other end has a
positive polarity.
• Polarity in Chemistry, well it is basically the separation
of an electric charge which leads a molecule to have a
positive and negative end
Polarity
66. •Non-polar Covalent bond
• When the 2 atoms having similar electronegativity will
share electrons equally.
•Polar Covalent bond
• when 2 bonded atoms are not equally distributed
• the electrons, one atom is more electronegative than
the other atom,
• this bond is polarized, meaning one atom is partially
positive and the other atom is partially negative.
71. In an H-F bond, the fluorine atom is said to be more
electronegative than the Hydrogen atom. The electrons
eventually spend more time at the Fluorine atom. Hence, this
F atom slightly becomes negative whereas the Hydrogen
atom tends to become slightly positive.
72.
73.
74. •The electronegativity difference can be
calculated by getting the electronegativity value of
the given molecules in the periodic table of
elements.
Type of Bond Based on
Electronegativity
75.
76. • Water is said to be a polar molecule due to the difference in the
electronegativities between the oxygen atom and the hydrogen.
Oxygen is a highly electronegative atom when compared to
hydrogen.
• Fats, petrol, oil, and gasoline are said to be non-polar
molecules as they do not dissolve in water and nonpolar is
insoluble in water.
Examples of Polar and Non-
Polar Molecules
82. 1. N (3.0) and H (2.1)
2. H (2.1) and H (2.1)
3. Ca (1.0) and Cl (3.0)
4. C (2.5) and S (2.5)
5. Mg (1.2) and O (3.5)
6. H (2.1) and F (4.0)
7. H (2.1) and Cl (3.0)
8. P (2.1) and s (2.5)
9. S (2.5) and O (3.5)
10. Cl (3.0) and Cl (3.0)
Ionic, Polar and Non-Polar
Covalent Compounds
(ionic)Ionic Compound, (polar) Polar and (non-polar) Non-Polar Covalent Compounds
84. 1. N (3.0) and H (2.1) = .9 polar
2. H (2.1) and H (2.1) = 0 non-polar
3. Ca (1.0) and Cl (3.0) = 2 ionic
4. C (2.5) and S (2.5) = non-polar
5. Mg (1.2) and O (3.5) = 2.3 ionic
6. H (2.1) and F (4.0) = 1.9 ionic
7. H (2.1) and Cl (3.0) = .9 polar
8. P (2.1) and s (2.5) = .4 non-polar
9. S (2.5) and O (3.5) = 1 polar
10. Cl (3.0) and Cl (3.0) = 0 non-polar
Ionic, Polar and Non-Polar
Covalent Compounds
(ionic)Ionic Compound, (polar) Polar and (non-polar) Non-Polar Covalent Compounds
86. Determine whether polar or non-polar the
following paired atoms. Then, arrange the
following bonds in order of increasing polarity.
1. C-O
2. P-S
3. C-S
4. Cl-Br
5. Br-F
88. Determine whether polar or non-polar the
following paired atoms. Then, arrange the
following bonds in order of increasing polarity.
1. C-O = Polar
2. P-S = Non-polar
3. C-S = Non-polar
4. Cl-Br = Non-polar
5. Br-F = Polar
CS 0
ClBr .2
PS .4
C0 1
BrF 1.2
89. The chemical bond between hydrogen and
oxygen in water is a:
A. Polar Covalent bond
B. Covalent Bond
C. Ionic bond
D. Metallic bond
90. What is the most electronegative element?
A. Chlorine
B. Flourine
C. Hydrogen
D. Carbon
91. The chemical bonds between hydrogen atoms
in a dihydrogen molecule are:
A. Polar Covalent bond
B. Non-Polar Covalent Bond
C. Ionic bond
D. Metallic bond
92. What type of bond does NO2 forms?
A. Ionic bond
B. Covalent bond
C. Coordinate covalent bond
D. Dative bond
94. 1. K—Cl
2. N—O
3. H—Cl
4. C—Br
5. C—O
Based on the electronegativity value, determine if
the following bonds are nonpolar,
polar, and ionic.
95. What I Have Learned
•Intramolecular forces are the attractions between atoms
•Intermolecular forces are the attractions between molecules
•Ionic bonds form when two oppositely charged atoms (called ions)
transfer their electrons (negatively charged particles) to create a secure
bond between the two.Most often, you’ll see this bond happen between a
metal and nonmetal.
•Covalent bonds are created when atoms share their electrons. Covalent
bonds happen between two nonmetals.
•Metallic bonds.Metal shares electrons with another metal.
96. What I Have Learned
•Cations. Positively charged ions
•Antions. Negatively charged ions
•Electronic Configuration. refers to the arrangement of the
electron within the orbitals of an atom to know more about an
atom’s electronic property.
•Valence electrons are the electrons located at the outermost
shell of an atom, involved in chemical bonding.
97. What I Have Learned
•Polar bond, there is an unequal sharing of electrons between and among atoms.
•In non-polar bond, there is an equal sharing of electrons between and among
atoms.
• Electronegativity is the ability of an atom in a molecule to attract electrons.
• As electronegativity increases, the attraction of the atom for electrons increases.
•The polarity is a result of uneven distribution of charges of atoms in a molecule.
•The non-bonding electrons are called lone pairs. The bonded electrons are called
bonding pairs.
Editor's Notes
Elements are pure substances which are composed of only one type of atom. Compound are substances which are formed by two or more different types of elements that are united chemically in fixed proportions.
Atoms are single neutral particles. Molecules are neutral particles made of two or more atoms bonded together. An ion is a positively or negatively charged particle.
