Ch. 11.4 Notes---Atomic Properties and the Periodic Table

1
Ch. 11.4 Notes---Atomic Properties and the
Periodic Table

• Valence Electrons and Electron Dot Notations
• What are valence electrons?
• These are the electrons in the
  _________-_______ energy level (or shell). These
  are responsible for chemical bonding.
• All of the other electrons are called core
  electrons.
• They will be ___ electrons and ___
  electrons only.
• Counting Valence Electrons
• Group A number of valence electrons
• (only exception Helium __ e-s)
• Examples Ca __ e-s Nitrogen __ e-s Argon
  __ e-s
• d-block and f-block ___valence e-s

outer
most
p
s
2
2
5
8
2
2
Drawing Valence Electrons

• Electron-dot notation Electrons will be
  represented as dots located around the symbol of
  the element in the pattern shown below.
• Examples Nitrogen Hydrogen
  
• (important exception.... Carbon )

X
3
6
1
4
7
2
5
8
N
H
C
3
The Development of the Periodic Table
Dmitri Mendeleev

• _________________________ constructed the 1st
  periodic table
• Features of Mendeleevs Periodic Table
• He left ______ _________ for missing
  elements. Later when these elements were
  discovered, he filled in the gaps.
• He arranged the elements in columns and rows
  according to their __________________. Elements
  with similar properties were in the same
  horizontal row.
• He was able to accurately ___________ the
  properties of the missing elements based on the
  properties of the elements in similar _______.
• He ordered the elements by increasing
  __________ ___________.

blank spaces
properties
predict
rows
atomic mass
4
Features of the Modern Periodic Table
Moseley

• In 1913, Henry ______________ determined the
  atomic number, ( of ___), of the elements.
• He then arranged the elements in the periodic
  table by increasing atomic ____________.
• This switched the position of some elements.
  This is how the modern periodic table is arranged
  today.
• Horizontal Rows ____________ or Series
• Vertical Columns ____________ or Families
• Elements in the same _________/_________ have
  similar properties.

p
number
Periods
Groups
groups
families
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Figure 11.35 Classification of elements as
metals, nonmetals, and metalloids.
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Parts of the Periodic Table
left

• Metals located to the _______ of the dark
  zig-zag line running through the p-block. This
  includes the elements in the ___-block.
• Properties of Metals
• shiny surface
• ______________ (you can pound it into a flat
  sheet)
• ______________ (you can draw it into a thin
  wire)
• good _______________ (heat/electricity travels
  through it easily)

f
malleable
ductile
conductors
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Parts of the Periodic Table

• Nonmetals located to the ___________ of the
  dark zig-zag line.
• Properties of Nonmetals
• _______ surface
• ______________
• good _______________ (or poor conductors)
• Metalloids located on the border of the dark
  zig-zag line.
• Examples Silicon Germanium
• Properties of Metalloids
• ___________________

right
dull
sulfur
brittle
insulators
semiconductors
(Used in computer chips)
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Parts of the Periodic Table

• d-block metals _________________ metals
• f-block metals Inner-transition metals or
  ____________ metals
• Special Group/Family Names
• Group 1A _________ metals
• React with _________ to form a base
• Group 2A ________________ metals
• Compounds are used in batteries
• Group 7A _________________
• Used in some light fixtures
• Group 8A (or 0 or 18) _______ gases
• Dont form compounds (_________)

transition
rare-earth
Alkali
water
Alkaline-earth
Halogens
Noble
inert
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Parts of the Periodic Table
Inner-transition metals
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Trends in the Periodic Table

• Atomic Size (Atomic Radius)
• (See Fig. 11.36)
• Moving Down a Group the size of the atoms
  ________________
• Why? You are adding ________ electrons to
  higher and higher energy levels (farther and
  farther out.)
• Moving Across a Period the size generally
  ______________
• Why? You are adding more e- and p to the same
  energy level. This causes more ______________
  of opposite charges and it __________ the
  electron cloud inward.

increases
more
decreases
attraction
pulls
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Figure 11.36 Relative atomic sizes for selected
atoms.
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Trends in the Periodic Table

• Atomic Size vs. Ion Size
• (See Figure 12.8)
• Cation (___) charged atom created by
  ___________ e-s.
• Cations are ______________ than the original
  atom.
• _____________ generally form cations.
• Anion (___) charged atom created by
  _____________ e-s.
• Anions are ____________ than the original atom.
• _______________ generally form anions.

removing
smaller
Metals
-
adding
larger
Nonmetals
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Trends in the Periodic Table

• Atomic Size vs. Ion Size

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Figure 12.8 Relative sizes of some ions and
their parent atoms.
picometers
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Trends in the Periodic Table

• Ionization Energy
• Ionization energy is the energy required to
  _______________ the outer most electron in an
  atom.
• Moving Down a Group _______________ (less
  energy is needed)
• Why? You are trying to remove an electron that
  is farther and farther out (for
  larger and larger atoms). These e-s
  are not as ________________to the nucleus.
• In general, the larger the atom, the ____
  attracted it is to its e-s.

remove
decreases
attracted
less
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Trends in the Periodic Table

• Ionization Energy
• Moving Across a Period generally
  ________________
• Why? Moving across a period takes us from
  metals to nonmetals. More ionization
  energy is needed for
  ______________ compared to __________.
• Also, since metals generally form _________, it
  wont take as much energy to remove its outer
  most electron.
• Remember that as you move across the period, the
  atoms get _________ and therefore ______
  attracted to the electrons.

increases
nonmetals
metals
cations
smaller
more
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First Ionization Energies
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Trends in the Periodic Table

• Successive Ionization Energies
• Successive Ionization Energies means the energy
  required to remove a _____ or a _____ electron
  from an atom.
• Removing more and more e-s requires ______ and
  ______ energy.
• Why? The remaining e-s are more _________
  _________ to the nucleus.

2nd
3rd
more more
tightly bound
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Trends in the Periodic Table

• Electronegativity
• (See Figure 12.4)
• Electronegativity is a relative value
  (from_________) which compares how much an atom
  is attracted to the e-s in a ____________ bond.
• Moving Down a Group generally ______________
  (less attraction)
• Why? The bonded electron is farther and farther
  out. These e-s will not be as
  attracted to the larger and larger
  atoms.

0 4.0
chemical
decreases
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Figure 12.4 Electronegativity values for
selected elements.
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Trends in the Periodic Table

• Electronegativity
• Moving Across a Period generally
  _________________
• Why? Again, the atoms are getting ________ so
  they are _______ attracted to the bonding
  electrons.
• Also, moving across a period takes us from
  metals to nonmetals. Since nonmetals generally
  form _________, they tend to __________ e-s
  anyway, and this makes them ________________
  attracted to e-s when forming a chemical bond.
• ___________ __________ are not listed in Figure
  12.4 since they do not ________ _____________ !

increases
smaller
more
anions
gain
highly
Noble gases
form compounds
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Determining the Ion Formed

• Atoms try to achieve a ________ ______
  configuration when forming an ion. (This makes
  them more stable.)
• Locate the nearest noble gas and count how many
  places it is away, but remember that you can
  skip over the d-block!!
• This amount will be the same as the of e-s
  either gained or lost by the atom when forming an
  ion.
• Practice Problem How many electrons are gained
  or lost when forming an ion from the following
  elements?
• a) Magnesium ____ (gained or lost) b) Iodine
  ____ (gained or lost)
• c) Gallium____ (gained or lost) d) Boron____
  (gained or lost)

noble gas
2
1
3
3