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Worksheetsexam1
Total questions: 27
Worksheet time: 28mins
match
Horizontal rows
periods
columns
groups
The distribution of electrons into the various
orbitals in an atom in its ground state is called its
electron configuration
The ground state of the electron is the lowest
energy orbital it can occupy.
Ground state
All electrons have the same amount
spin
Match
The orientation of the electron spin is
Quantized(only one direction or oppisit)
adds a fourth quantum number to the
description of electrons in an atom
electron spin
spin quantum number
ms
No two electrons in an atom may have the same set of four
quantum numbers.
pauli exclusion
umbers.
• Therefore, no orbital may have more than two electrons,
and they must have opposite spins.
pauli exclusion
Match
more than one orbital of the same
energy is available, the electron will occupy
an unfilled orbital first before pairing up.
hunds rule
Orbitals fill from lowest energy to
highest.
Afbau principle
The electrons in the outermost principal energy level
are called the
Valence electrons
Valence electrons dictate the
behavior and reactivity of elements
All the other electrons are called
Core electrons
match
formed when atoms lose or gain
electrons
Ions
have 8 valence electrons which
makes them stable
noble gases
loses valence electrons
cation
Oxygen atom has six valence electrons.
becomes O2− anion = 1s22s22p6
x-
anion
match
X+
cation
If an atom/ion has unpaired electrons
paramagnetic
paramagnetic
attracted to a magnet field
no unpaired electrons
diamagnetic
always form positively charged
cations
match
form negatively charged anions
Nonmetals
an average
radius of an atom based on
measuring large numbers of
elements and compounds.
atomic radius
atomic radius increases
from top to bottom
atomic radius decreases
from left to right
if cations are smaller than neutral atom
anions are larger
Match
minimum energy needed to remove an
electron from an atom or ion in the gas phase.
Ionization energy
Left to right increase
ionization energy except 5a-6a
s-sublevel can hold 2
electrons
p sublevel
can hold 6 electrons
can hold 10 electron
d sublevel
match
D block
transition metal
halogens
non metals
Ion size increases
Down a column
Valence electrons are held
loosely
Sodium has only one valence electron that is easily
removed;
becuase its in group 1
Exceptions
cr
Mo
Cu
Ag
match
Atoms that have a high electronegativity
Hold on to their electrons more tightly
traveling down the table increases
the atomic radius
traveling left increases
atomic radius
outer most shell level
valence electrons
React high
alkali earth and halogens
Match
as you move across the periodic table atoms tend to get smaller because
the atoms have more protons
the ability to accept/attract electrons
electronegativity
Traveling across the atomic radius
decreases
ionization energy increases towards
flourine
as you move down atoms get bigger because
energy levels
match
Energy required to remove an electron from an atom
ionization energy
electro negativity decreases
from top to bottom
the tendency of An atom to attract electrons and acquire a negative charge
electronegativity
Which of the following will have a higher electronegativity than arsenic
C
Ne
Sb
Ge
Metal
ductile
conductor
shiny
lust
Electricity and heat
What is the element with the highest metalllic?
Fr
Cs
energy change that occurs when an atom gains an electron.
Electron affinity
electronegativity
Exception
Chlorine has a greater electron affinity than F
T
F
1st IE 496, 2nd 4560 (big jump), 3rd IE 6910
big jump 1 to 2
big jump 2 to 3
Match
The more energy that is released
the larger the electrons ffinity
the more negative number
the larger the electron affinity
the energy change associated with the addition of an electron to a gaseous atom
electron affinity
Ionization energy exceptions
Be
N
O
B
match
Minimum energy needed to remove an electron from an atom or ion in the gas phase
ionization energy
Ionization energy
always endothermic
endothermic
requires energy to remove an E
generally
1st IE<2nd IE< 3rd IE
Mg 2+ , Na+ Ne , F-
in order by increasing size
in order by atomic number
in order by energy
The Samar number of electrons
isoelectronic
anion
electonegativity
cation
If cation are smaller than neutral atoms, (a) are larger than neutral atoms
For iselectronic species, greater the nuclear charge,
bigger the atom
smaller the atom
When atoms for anions electrons are
added
substracted
The positive charge “felt” by an electron relative to other electrons
atomic radii
z eff
ionization
