National University
CAHINORC - INORGANIC AND ORGANIC CHEMISTRY [LEC]
NUR255
Name: Zardy Gabriel N. Andaya
CORNELL NOTES 3.1
LEARNING OBJECTIVES Notes
Discuss the trends in the
periodic table of element and
their properties.
Differentiate metals from
nonmetals. PERIODIC TRENDS
What is electronegativity? Electronegativity
‒ Refers to the the measure
of an atom’s tendency to
attract a bonding pair of
electrons.
Does Electronegativity Electronegativity increases across
a period, and increases up a
increases across a period?
group, with fluorine being the
most electronegative atom.
What is Ionization energy? Ionization energy
‒ Refers to the amount of
energy required to remove
the most loosely bound
electron of a neutral atom.
Does electrons near the Electrons that are closer to the
nucleus need more energy to nucleus are going to be more
be tightly held? tightly held than those that are
further away and will require
more energy to pull them off the
atom.
REFLECTION
Electronegativity refers to the measure of an atom’s tendency to attract
electrons, while Ionization energy refers to the amount of energy required
to remove the most loose electrons in a neutral atom.
Electrons that are closer to the nucleus are going to be more tightly held.
, PROPERTIES OF
ELECTRONEGATIVITY OF
ELEMENTS:
How high the electronegativity Small atomic radius = High
and ionization energy of a electronegativity and high
small atomic radius? ionization energy.
How low the electronegativity Large atomic radius = Low
and ionization energy of a electronegativity and low
large atomic radius? ionization energy
METALLIC PROPERTIES
Metallic Properties
‒ Refer to the physical and
What are metallic properties? chemical characteristics
commonly observed in
metals due to the nature of
metallic bonding.
What is the arrangement for In metallic properties, positive
positive metal ions? metal ions are arranged in a
regular lattice.
The structure of metallic bonds are
What is the structure of not held by any specific atom
metallic bonds? wherein the structure of their
valence electrons forms a
somewhat "sea of electrons".
What is the purpose on why The structure of metallic bonds
metallic bonds are arranged gives metals:
like a sea of electrons?
• Flexibility (without
breaking bonds)
• High electrical / thermal
conductivity
• Strong internal cohesion
REFLECTION
Properties of Electronegativity of Elements: Small atomic radius = High
electronegativity and high ionization energy, while Large atomic radius =
Low electronegativity and low ionization energy.
CAHINORC - INORGANIC AND ORGANIC CHEMISTRY [LEC]
NUR255
Name: Zardy Gabriel N. Andaya
CORNELL NOTES 3.1
LEARNING OBJECTIVES Notes
Discuss the trends in the
periodic table of element and
their properties.
Differentiate metals from
nonmetals. PERIODIC TRENDS
What is electronegativity? Electronegativity
‒ Refers to the the measure
of an atom’s tendency to
attract a bonding pair of
electrons.
Does Electronegativity Electronegativity increases across
a period, and increases up a
increases across a period?
group, with fluorine being the
most electronegative atom.
What is Ionization energy? Ionization energy
‒ Refers to the amount of
energy required to remove
the most loosely bound
electron of a neutral atom.
Does electrons near the Electrons that are closer to the
nucleus need more energy to nucleus are going to be more
be tightly held? tightly held than those that are
further away and will require
more energy to pull them off the
atom.
REFLECTION
Electronegativity refers to the measure of an atom’s tendency to attract
electrons, while Ionization energy refers to the amount of energy required
to remove the most loose electrons in a neutral atom.
Electrons that are closer to the nucleus are going to be more tightly held.
, PROPERTIES OF
ELECTRONEGATIVITY OF
ELEMENTS:
How high the electronegativity Small atomic radius = High
and ionization energy of a electronegativity and high
small atomic radius? ionization energy.
How low the electronegativity Large atomic radius = Low
and ionization energy of a electronegativity and low
large atomic radius? ionization energy
METALLIC PROPERTIES
Metallic Properties
‒ Refer to the physical and
What are metallic properties? chemical characteristics
commonly observed in
metals due to the nature of
metallic bonding.
What is the arrangement for In metallic properties, positive
positive metal ions? metal ions are arranged in a
regular lattice.
The structure of metallic bonds are
What is the structure of not held by any specific atom
metallic bonds? wherein the structure of their
valence electrons forms a
somewhat "sea of electrons".
What is the purpose on why The structure of metallic bonds
metallic bonds are arranged gives metals:
like a sea of electrons?
• Flexibility (without
breaking bonds)
• High electrical / thermal
conductivity
• Strong internal cohesion
REFLECTION
Properties of Electronegativity of Elements: Small atomic radius = High
electronegativity and high ionization energy, while Large atomic radius =
Low electronegativity and low ionization energy.
