The Periodic Table- Topic 5

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Homework 1. Read pages 78-83 in RB complete
1-29 on separate paper (read carefully)2.
Complete guide pg 4 (use your periodic table and
colored pencils/crayons)

• The Periodic Table- Topic 5

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Mendeleevs Periodic Table (1869)
6.1
Searching For an Organizing Principle

• How did Mendeleev organize his periodic table?
• The Abbreviated History of the Periodic Table for
  Regents Chemistry

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A. Dmitri Mendeleev (1869, Russian)
I. HISTORY

• Organized elements by
• increasing ATOMIC MASS.
• Elements with similar chemical properties were
  grouped together.
• There were some discrepancies.

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B. Henry Moseley

• ORGANIZED ELEMENTS BY INCREASING ATOMIC NUMBER.
• Resolved discrepancies in Mendeleevs
  arrangement.
• The modern periodic table known as The Periodic
  Law

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• When elements are arranged in order of INCREASING
  ATOMIC , elements with similar chemical
  properties appear at regular intervals.
• The properties of the elements within a period
  change as you move across a period from left to
  right.
• The pattern of properties within a period repeats
  as you move from one period to the next.

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II. ORGANIZATION OF THE ELEMENTS
A. Arrangement of Table

• 1. Horizontal rows
• Called PERIODS
• All elements in the same period have the same
  number of ENERGY LEVELS in their atomic structure
• 7 periods/energy levels

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2. Vertical Columns

• Called GROUPS OR FAMILIES
• All elements in the same group have the
• same number of VALENCE ELECTRONS, therefore
  lose or gain the SAME number of electrons, form
  similar CHEMICAL FORMULAS and have similar
  CHEMICAL PROPERTIES
• ex. XCl2 Group 2
• Be2 Cl-1
• Mg2 Cl-1

• When writing formulas, use the criss-cross rule
  to cancel out oxidation states

BeCl2
MgCl2
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III. Comparing Metals, Nonmetals Metalloids
Elements on the Periodic Table are divided into
three subgroups called METALS, NONMETALS and
METALLOIDS (semimetals).
Nonmetals on the right
Metals on the left
Metalloids (touch the staircase)
Group 18 are Noble Gases
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Record metallic properties i
Increase nonmetallic properties
Decrease metallic properties
Increase metallic properties
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METALS located on the LEFT SIDE of the
periodic table (except H) MORE THAN 2/3 of all
elements

• Table J  Activity Series                    
                                 

• 1. Chemical properties
• tend to LOSE ELECTRONS EASILY (radius gets
  smaller)
• have LOW IONIZATION ENERGY (energy needed to
  remove electrons)
• Metallic character INCREASES as ionization energy
  decreases.
• have a low electronegativity (attraction for
  electrons)
• form POSITIVE IONS (cations) when combining with
  other atoms
• FRANCIUM most reactive metal See Table J

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2. Metal Physical Properties

• good conductors of heat and electricity due to
  their mobile valence electrons
• LUSTROUS - reflect light, shine when they are
  polished
• MALLEABLE - can be rolled or hammered into
  sheets
• DUCTILE - can be drawn into wires
• are SOLIDS at room temperature except for
  MERCURY (liquid)

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B. NONMETALS- located on the right side of the
periodic table (except for Noble gases)

• Table J  Activity Series                    
                                 

• Chemical properties
• tend to GAIN electrons to form negative IONS
  (anions) resulting in a larger radius
• have high electron affinities (electronegativity)
• produce COVALENT bonds by SHARING electrons with
  other nonmetals
• FLUORINE most reactive nonmetal see Table J

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• 2. Nonmetals Physical Properties
• exist as gases, molecular solids, or network
  solids at room temperature except BROMINE
  (liquid)
• BRITTLE - (shatters when struck)
• DULL - does not reflect light even when polished
• POOR CONDUCTORS of heat and electricity
• Allotropes Different SHAPE PROPERTIES forms
  from the same element.
• CARBON coal diamond, graphite
• OXYGEN O2 O3 (OZONE)

Know this definition examples
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Crystal Structure and Unit Cells

• 13.3

• Carbon Allotropes

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C. METALLOIDS (semi-metals)

• Found lying on the jagged line between metals and
  nonmetals flatly touching the line (except Al and
  Po).
• B, Si, Ge, As, Sb Te
• Exhibit properties of both metals and nonmetals
• Behave as nonmetals but their conductivity is
  like metals
• SEMICONDUCTORS Si and Ge

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Buckminsterfullerene

• The structure of a buckminsterfullerene is a
  truncated icosahedron made of 20 hexagons and 12
  pentagons, with a carbon atom at the vertices of
  each polygon and a bond along each polygon edge.
  To become stable, the carbon atom needs 8
  electrons in its outer shell, and covalently
  bonding with 3 other atoms will only make 7
  electrons in its outer shell. This means that the
  one unbonded electron on every carbon atom is
  free to float around all of the compound's atoms.
  Electrons carry charge, so this free electron
  movement means that the buckminsterfullerene can
  conduct electricity very well. This, because of
  its size, makes it very useful in nanotechnology.

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Squares in the Periodic Table
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Trends in the Periodic Table

• Many properties of the elements change in a
  predictable way as you move through the periodic
  table these systematic trends are called
  periodic trends. (use reference Table S for data
  comparison)

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IONIZATION ENERGY (IE)

• Energy needed to remove the most loosely bound
  electron from a neutral gaseous atom
• X energy X e-
• Atoms with a HIGH ionization energy hold onto
  electrons MORE EASILY and are less likely to give
  them up.
• Atoms with a LOW Ionization Energy hold onto
  electrons LOOSELY and are more likely to LOSE
  electrons

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• IE TREND GOING ACROSS A PERIOD
• What is the trend as you move left to right? IE
  INCREASES
• Explanation AS THE PROTONS (AKA NUCLEAR
  CHARGE) INCREASES, THERE IS A GREATER PULL ON THE
  ES REQUIRING MORE NRG TO REMOVE THEM
• IE TREND GOING DOWN A GROUP OR FAMILY
• What is the trend as you move top to bottom? IE
  DECREASES
• Explanation Atom size increases making the
  outermost electron farther away from the nucleus
  therefore making it easier to remove
• Shielding increases

INCREASES
DECREASES
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Trends in Ionization Energy
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Trends in Ionization Energy
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Trends in Ionization Energy
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Atomic Radii

• one half of the distance between the nuclei of
  two atoms of the same element when the atoms are
  joined.

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AR TREND in a period

• As you move across left to right on a table,
  values generally DECREASES
• Why? THE GREATER THE PROTONS (atomic ), THE
  STRONGER THE PULL ON THE ES BRINGING THEM CLOSER
  INTO THE NUCLEUS

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AR TREND GOING DOWN A GROUP OR FAMILY

• Atomic radii generally INCREASES from the top of
  the table to the bottom of the table
• Why? Due to electron shielding As you move down,
  YOU ADD ANOTHER NRG LEVEL INCREASING THE
  SHIELDING (KERNEL E- BLOCK)

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IONIC RADIUS (write on the bottom of your
page)

• A LOSS OR GAIN IN ELECTRONS BY AN ATOM WILL
  CHANGE THE SIZE OF THE RESULTING ION
• Metals lose es resulting
• in smaller ionic radius
• Nonmetals gain es resulting
• in larger ionic radius

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Trends Relative Sizes of Some Atoms and Ions
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COMPARISON OF METALS TO NONMETALS

• If you generally compare ionic size for metals
  and nonmetals, metal ionic sizes are SMALLER and
  nonmetal ionic sizes are BIGGER.
• This is because metals tend to LOSE electrons and
  form CATIONS (and get smaller) while nonmetals
  tend to GAIN electrons and form ANIONS (and get
  larger).

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• METALS TREND GOING ACROSS A PERIOD
• Trend As you move left to right for METALS,
  ionic size DECREASES
• Explanation METALS LOSE ELECTRONS FROM THEIR
  OUTERMOST SHELL
• METALS TREND GOING DOWN A GROUP
• Trend As you move down a group for METALS, ionic
  size INCREASES
• Explanation AS YOU MOVE DOWN A GROUP, YOU ADD
  ANOTHER ENERGY LEVEL THEREBY INCREASING THE
  SIZE DUE TO THE INCREASED OF ELECTRONS

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• NONMETALS TREND GOING ACROSS A PERIOD
• Trend As you move left to right for NONMETALS,
  ionic size decreases.
• Explanation NONMETALS GAIN ELECTRONS WHICH ARE
  ATTRACTED TO THE PROTONS IN THE NUCLEUS
• NONMETALS TREND GOING DOWN A GROUP
• Trend As you move down a group for NONMETALS,
  ionic size INCREASES.
• Explanation AS YOU MOVE DOWN A GROUP, YOU ADD
  ANOTHER ENERGY LEVEL THEREBY INCREASING THE SIZE
  DUE TO THE INCREASED OF ELECTRONS

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ELECTRONEGATIVITY (EN)

• Description MEASURE OF AN ATOMS ABILITY TO
  ATTRACT ELECTRONS
• Atoms with a HIGH Electronegativity have a
  STRONGER attraction for bonded electrons
• Atoms with a LOW Electronegativity have a WEAKER
  attraction for bonded electrons
• Based on a scale of 4, Fluorine has the greatest
  EN

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• EN TREND ACROSS A PERIOD
• What is the trend as you move left to right?
• INCREASES
• Explanation THERE ARE MORE PROTONS (INCREASED
  ATOMIC NUMBER) WHICH INCREASES THE ELECTRONS
  ATTRACTION

• EN TREND GOING DOWN A GROUP OR FAMILY
• What is the trend as you move top to bottom?
• DECREASES
• Explanation AS YOU GO DOWN A GROUP THERE ARE
  MORE ELECTRONS AND MORE NRG LEVELS SO THE
  ATTRACTION GETS WEAKER

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Periodic Trends Summary(use reference Table S
for data comparison)
Trend Across a period Down a group
Ionization energy increases decreases
Electronegativity increases decreases
Atomic radii decreases increases
Metallic properties decreases increases

• Click on for video clip

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Class/Home work - Trends

• Class work Complete guide pg 8
• Only collect trend data for groups 1 and 7, and
  periods 2 and 4
• Complete pgs 10-11 in guide
• Visit my website for on-line practice with the
  trends and the PT vocabulary
• Trends Quiz Friday
• Bring Review books to class tomorrow

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IV. Classification

• Alkali Metals
• Alkaline Earth Metals
• Transition Metals
• Halogens
• Noble Gases

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Group 1 Alkali Metals

• extremely reactive (not found free in nature)
  -form stable ionic compounds
• react with water to form a base
• react with air to form oxides
• react with acids to form salts

Click on for video clip (256 min)
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Group 2 Alkaline Earth Metals

• reactive (not found free in nature) - form stable
  ionic compounds
• react with water to form a base
• react with air to form oxides
• react with acids to form salts

Click on for video clip
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Groups 3-11 Transition Metals

• multiple positive oxidation states
• Lose electrons from two outermost energy levels
• Ions form colored solutions
• Ex. CuSO4 (due to the Cu 2 ion)

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Group 15 unique features

• Members range from typical nonmetals (nitrogen
  and phosphorus) through metalloids (arsenic and
  antimony) to metals (bismuth)
• Nitrogen
• Forms stable diatomic molecules with a triple
  bond
• Component of protein
• Forms some unstable compounds that are used as
  explosives
• Phosphorus
• Component of nucleic acids (DNA, RNA)
• More reactive than nitrogen at room temperature

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Group 16 unique Features

• Members range from typical nonmetals (oxygen and
  sulfur) through metalloids (selenium and
  tellurium) to metals (polonium)
• Solids except oxygen
• Oxygen can exist as O2 and O3 (it is an
  allotrope)
• Polonium is radioactive

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Group 17 Halogens

• very reactive nonmetals - high electronegativity
• not found free in nature
• form diatomic molecules when free
• react with metals to form salts (halides)
• Found in all three phases (s, l, g) due to
  differences in Van der Waals forces (these are
  weak)

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Group 18 Noble Gases

• Have complete outer shells
• Almost inert (not reactive) stable
• Krypton, xenon, and radon form compounds with
  oxygen and fluorine
• Referred to as monatomic gases

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TODAY PT Day 1

• 1. Check HW answers on the side board. Record
  correct answers in RB turn in HW.
• 2. Jigsaw
• Report to your colored groups and BEGIN your PT
  teachback.
• Present (teach) your information to the group
  FIRST! This NOT a silent lesson use your 6
  inch voices to teach the other members.
• Complete the section of notes cooperatively. Ask
  your questions to ascertain clarity.
• By Day 2, everyone in the group should have the
  Teachback WS completed and the follow-upo
  questions started.
• Cooperation and diligence is necessary..
• I will be watching and listening.

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Today PT Day 2

• Continue with your group teach back then proceed
  to answer/check questions 46-90. Transfer
  answers to the sheet provided.
• Answers to the outline are on my website for YOU
  to review this evening.
• Transfer s 46-74 to the scantron. On the
  scantron write Periodic Table Teachback
• Due Thursday BOTH the answer sheet, scantron,
  and each members research notes.
• Group Quiz THURSDAY

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Today PT Day 3

1. Transfer s 46-74 to the scantron beginning with
   46 on the scantron. Record all group members
   names in the name section. In the subject area,
   write PT Teachback.
2. Group quiz each member should record his/her
   answers on their own quiz paper. I will collect
   one random quiz to score. Work together.
3. Transfer quiz responses 1-21 to the same
   scantron.
4. Submit the following
5. Answer sheet
6. Scantron (1-21 and 46-74 recorded)
7. Each members research notes.

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TEACHBACK PROJECT REVIEW

• Alkali Metals
• Alkaline Earth Metals
• Transition Metals
• Halogens
• Noble Gases

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GROUP 1
video

• 1. The name of this group is ALKALI METALS
• 2. Does this group contain metals or nonmetals?
  METALS
• 3. Alkali metals (lose or gain)l LOSE electrons
  becoming (positive or negative) ions? POSITIVE
• 4. Describe the reactivity of the elements in
  this group as the atomic number increases.
  INCREASES
• 5. Are they (more or less) MORE reactive than all
  of the elements in Group 2 and why? THEY HAVE
  LOWER IONIZATION ENERGIES

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Group 1 continued

• 6. Can these compounds be found in nature in the
  elemental or combined state? COMBINED STATE IN
  THE FORM OF A SALT
• 7. What type of compounds do they normally form
  (ionic or covalent)? IONIC (M NM)
• 8. If element Y represents an alkali metal, what
  is its general formula for the reaction with a
• Chloride YCl Oxide Y2O
• 9. What is the most reactive metal in this group?
  FRANCIUM

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GROUP 2
video

• 1. The name of this group is ALKALINE EARTH
  METALS.
• 2. Does this group contain metals or nonmetals?
  METALS
• 3. They (lose or gain) LOSE electrons form
  (positive or negative) ions POSITIVE ?
• 4. Describe the reactivity of the elements in
  this group as the atomic number increases
  (increases or decreases) DECREASES
• 5. Are they (more or less) LESS reactive than all
  of the elements in Group 1 and why? THEY HAVE A
  GREATER IE

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Group 2 continued

• 6. Can these compounds be found in nature in the
  elemental or combined state? COMBINED STATE IN
  THE FORM OF A SALT
• 7. What type of compounds do they normally form
  (ionic or covalent)? IONIC (M NM)
• 8. If element Z represents an alkaline earth
  metal, what is its general formula for the
  reaction with a
• Chloride ZCl2 Oxide ZO

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GROUP 15

• 1. What is this group referred to as? NITROGEN
  GROUP
• 2. Name the diatomic element in this group?
  NITROGEN
• 3. Classify each element in this group as a
  metal, non-metal or semi-metal (metalloid).
• metals ANTIMONY, BISMUTH
• nonmetals NITROGEN, PHOSPHORUS
• semi-metal ARSENIC
• 4. Explain what happens to the reactivity of a
  non-metal as the atomic number increases.
  DECREASES .
• 5. Which is the most reactive non-metal in this
  group? PHOSPHORUS
• 6. Is nitrogen a (diatomic or monatomic) DIATOMIC
  molecule what type of bond is found in
  nitrogen? TRIPLE COVALENT

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GROUP 16

• 1. Classify each element in this group as a
  metal, non-metal or semi-metal.
• metals POLONIUM nonmetals OXYGEN, SULFUR,
  SELENIUM semi-metal TELLERIUM
• 2. Name the diatomic element in this group.
  OXYGEN
• 3. Define an allotrope? DIFFERENT FORMS OF AN
  ELEMENT IN THE SAME PHASE WITH HAVING DIFF CHEM
  PHYSICAL PROPERTIES
• 4. Which element(s) in this group is an
  allotrope? SULFUR, OXYGEN (O2 and O3)
• 5. What type of element is Polonium? RADIOCATIVE
  METAL How can you tell it is radioactive? ITS
  ATOMIC NUMBER IS GREATER THAN 83

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TRANSITION ELEMENTS (groups 3B-12)

• Which element is a liquid at room temperature?
  MERCURY (Hg)
• 2. What are the four main characteristic chemical
  properties of transition elements?
• MULTIPLE POSITIVE OXIDATION STATES
• IONS FORM COLORED SOLUTIONS
• LOSE ELECTRONS FROM TWO OUTERMOST ENERGY LEVELS
• UNFILLED D ORBITALS

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GROUP 17

• 1. The name of this group is HALOGENS
• 2. Name and classify the elements in this group
• METALS At NONMETALS F, Cl, Br, I
• 3. Halogens (lose or gain) GAIN electrons
  becoming (positive or negative) ions? NEGATIVE
• 4. Why is astatine not included much in these
  discussions? NOT ENOUGH AVAILABLE TO STUDY
• 5. What would the general formula of a Group 17
  element (represented by X) combined with
  magnesium of
• group 2? MgX2

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• 6. What is the most reactive element in this
  group? FLUORINE
• 7. Can these compounds be found in nature in the
  elemental or combined state? COMBINED STATE AS
  SALTS
• 8. What type of salts do these elements form?
  HALIDES
• 9. For each state of matter, list the element(s)
  in this group. solid IODINE liquid BROMINE
  gas CHLORINE, FLUORINE
• 10. What type of forces of attractions account
  for the different states of matter that exist and
  the high MPs and BPs as you go down the group?
  VAN DER WAALS FORCES (weak forces that get
  stronger as you go down the group )

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GROUP 18

• The name of this group is called NOBLE GASES.
• What type of molecules do these gases form?
  (monatomic or diatomic) MONATOMIC
• Describe the electron arrangement in the
  outermost energy level of all these elements.
  STABLE OCTECT INERT GAS STRUCTURE
• Which element has only two electrons? HELIUM
• Describe the reactivity of the elements in this
  group. THEY ARE UNREACTIVE (Kr and Xe can be
  forced to react with F in lab settings)

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Topic 5 RB ANSWERS 46-90
56) _2__ 57) _3__ 58) _3__ 59) _2_ 60) _1__
46) _2_ 47) _1_ 48) _4_ 49) _1_ 50) _1_
66) _1_ 67) _2_ 68) _2_ 69) _4_ 70) _1_
61) _3_ 62) _3_ 63) _1_ 64) _1_ 65) _3_
51)_ 2_ 52) _4_ 53)_4_ 54) _3_ 55) _2_

• 71) _1_
• 72) _3_
• 73) _1_
• 74) _2_

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• 79) They both follow the octet rule (8 valence
  es)
• 80) Bromine MBr3 Oxygen M2O3 Why? Group 13
  has 3 valence es and will form a 3 charge
• 81) Hydrogen is a NM doenst have the
  characteristics of other group 1 members other
  than one valence e
• 82) LARGEST aluminum SMALLEST carbon
  
• HIGHEST IE carbon LOWEST IE
  aluminum
• 83) Same number of valence es
• 84) Metals have fewer valence es. As you move to
  the right of the PT, there are more val es. Once
  the orbitals are full, a noble gas configuration
  is met (8 val es)
• 85) Metals become positive ions
• 87) MCl2 88) MgX2 89) X2O