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2.5 Trends in periodic table
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2.5 part 2
Chemistry textbook > 2.5 Trends in periodic table
4 cards
Cards (28)
Electronegativity is...
the electron-attracting power of an atom
first ionisation energy
is...
the energy required to remove one electron from an atom
of an element in the gas phase.
periodicity is
a
repeating
pattern
What is effective nuclear charge also referred as?
Core charge
What is effective nuclear charge?
Is a measure of the
attractive force
felt by the
valence shell electrons
towards the
nucleus
number of protons in the nucleus - number of total inner-shell electrons: is the formula for?
Effective nuclear charge
The effective nuclear charge down a group....
Remains constant.
The effective nuclear charge left to right across a period....
increases
Electronegativity
is the
ability
of an
atom
to ....
attract electrons towards itself when
forming
a
chemical bond.
Electronegativity
is a measure of...
how strongly an atom pulls on the
electrons
of nearby atoms
Electronegativity down a group ...
decreases
From left to right electronegativity ...
increases
Atomic radius
is a measurement used for...
the size of atoms
Atomic radius can also be regarded as...
the distance from the nucleus to the valence shell electrons.
How is
atomic radius
measured?
By
halving
the
distance
between
the
nuclei
of
two atoms
of the same
element
that are
bonded together
Atomic radius
decreases
across a
period
as ...
effective nuclear charge increases
Atomic radius
down a group...
increases
Atomic radius
across a group (left to right)
decreases
What is
first ionisation energy
?
Is the
energy required
to
remove
one
electron
from an
atom
of a
element.
The
magnitude
of the
first ionisation energy
reflects how strongly...
the
valence electrons
are
attracted
to the
nucleus
of the
atoms
The more stronger the
valence electrons
are
attracted
to the
nucleus....
the
more energy
is
required
to
remove one
of them from the
atom
, and the
higher
the
first ionisation energy
First ionisation energy down a group...
decreases
The first ionisation energy left to right across a period....
increases
Metal reactivity down a group
increases
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