Chemistry - Chapter 2

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Chemistry - Chapter 2

• Inorganic Chemistry
• Quiz Friday 9/17/10
• 2.1 - 2.8

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Chemistry concept map 9/13/10

• Finding..Whats Matter?
• Hand-out Matter Concept map
• A FIELD STUDY
• Look around the room and on campus
• List 50 examples of matter
• Use your examples to explain matter?
• Write the definition of matter

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Periodic Table of Elements -handout
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What is matter made up of ? 9/14

• Elements, Atoms, Molecules, Compounds
• What is a chemical element?
• List the four most common elements found in
  living things.
• Atoms of what? Define atom.
• What are the subatomic particles of every atom?

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Chemistry explained

• Chemical Element - substance consisting of only
  ONE type of atom
• Most common C, H, O, N - (page 19)
• ATOMS of ELEMENTS.
• Atom - basic unit of matter
• Subatomic particles Protons (), neutrons
  (neutral charge), and electrons (-)
• Worksheet ATOMS Family

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8 O Oxygen 15.9998
Atomic number equals the number of _________or
__________ Atomic mass equals the number
of __________ __________
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8 O _______ 15.999
Atomic ______ Atomic Mass _________ of
Protons ________ of Neutrons ________ of
Electrons ________
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Atoms - Video making an atom 9/15
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• Atomic Structure draw and label the
• structure of the Carbon-12 atom
• on the template provided.
• Include nucleus, protons, neutrons, electrons,
  and energy levels.
• Indicate the charge on each
• DEFINE Atomic mass (mass number), Atomic number,
  atomic weight

C
CARBON
12.011
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CARBON - stable state

SUBATOMIC PARTICLES

• 6 PROTONS ()
• 6 NEUTRONS (neutral- no charge)
• 6 ELECTRONS (-)
• 2 ENERGY LEVELS - electron shells (level)
• UP to 2 ELECTRONS IN THE FIRST ENERGY LEVEL
• UP TO 8 ELECTRONS IN THE SECOND ENERGY LEVEL
  Carbon has 4

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Defined..

• Atomic mass (mass number) - sum of the protons
  and neutrons
• Atomic number - number of protons (unique for all
  atoms)
• Atomic weight - an elements atomic mass
• Worksheet Making calculations

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Molecules Compounds 9/16

• What is an isotope? How is it different than
  another atom of the same element?
• Draw and Complete the chart below

Element/Atomic Mass protons electrons neutrons Atomic mass
Carbon-12
Carbon-13
Carbon-14
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Warm-up 9/16/10

• Isotope different form of an element. Same
  number of protons and electrons, different number
  of neutrons

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ISOTOPES

• Isotope atom of an element that has a
  different number of electrons than that of
  the another atom of the same element

Protons (?) Electrons ( -?) Neutrons (neutral) Atomic mass
Carbon-12 6 6 6 12
Carbon-13 6 6 7 13
Carbon-14 6 6 8 14
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Could we shareplease!! 9/16

• Chemical bonds
• What is the difference between a covalent bond
  and an ionic bond?
• Valence electron - outer most energy level
  electrons
• Ion charged particle ( number of protons are
  not equal to the number of electron)

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Predict the number of valence electrons for each
element based on its location in the Periodic
Table of Elements. You will need to use the table
in your composition book. Barium _____ Lead
_____Sodium _____ Potassium ____
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LEWIS DOT STRUCTURES
ELEMENT ATOMIC OF PROTONS OF ELECTRONS OF VALENCE ELECTRONS
CHLORINE (Cl)
HYDROGEN (H)
SODIUM (Na)
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Lewis Dot Structures- Chemical Bonding

• Lewis Dot Structure Examples Step-By-Step
• Example 1 NaCl
• Step 1 ONLY USE VALENCE ELECTRONS
• Step 2 Arrange the atoms Na and Cl with their
  valence electrons represented as DOTS
• Step 3 Move electrons from the atom with the
  least number to the atom with the most number of
  electrons until they reach 8 (octet) total
  electrons ( 2 fro Hydrogen)

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Molecules and Compounds

• Define a molecule. Give three examples
• Define compound. What is the difference between a
  molecule and a compound?

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Defined..

• Molecule Two or more elements held together by a
  covalent bond
• EXAMPLES H2 ,O2 , H2O , CH4 (page 23)
• Compound - chemical composition of two or more
  elements in a fixed ratio
• EXAMPLES H2O , CaCl2, NaCl

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Definitions..

• Covalent bond - bond formed by the sharing of
  electrons ( )
• ionic bond - bond formed when one or more
  electrons are transferred from one atom to
  another - form ions

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Ionic and Covalent Bonding

• DIRECTIONS
• Each student will get 6 pieces of candy that will
  represent your VALENCE electrons 2 paper
  plates. DO NOT EAT YOUR CANDY!
• Using your paper plate, draw and color your atom
  assigned listed below add charges
• Activity 1 - covalent bonding
• Seats 1 - 24 draw an oxygen atom candy will
  represent your valence electrons (6)
• Seats 25 - 34 draw a Hydrogen atom candy will
  be your valence electrons (1)
• Seats 35 36 Draw a carbon atom candy will be
  your valence electrons (4)

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Chemical Bonding Covalent bonds

• Students will be given a chemical compound to
  produce with their classmates. You will be given
  three minutes to find your chemical element(s)
  and BOND to make one of the compounds listed
  below. Using your atom(plate) and electrons
  (candy) show how you are sharing to make a
  stable atom.
• O2 H2 H2O CH4
• (3) (4) (4) (2)

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Chemical bonding. Ionic bonds

• Using you second paper plate, draw your atom
  assigned below. You will now be producing IONIC
  bonds. One student will be giving away their
  electrons (candy), the other will gain
  electrons (candy).
• Seats 1 - 23 Chlorine (Cl)
• Seats 24 - 29 Sodium (Na)
• Seats 30 - 33 Calcium (Ca)
• Seats 34 - 36 Aluminum (Al

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Ionic bonds

• One student will be giving away their candy
  (electrons), the other will gain the candy
  (electrons). You will be given three minutes to
  find your chemical element(s) and BOND to make
  one of the compounds listed below. Use your atom
  (plate) and valence electrons (candy) to show how
  an ionic bond occurred.
• NaCl CaCl2 AlCl3
• (6) (4) (3)

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Properties of Water 9/17/10

• Quiz - 2.1 - 2.8

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Properties of Water 9/20/10

• Warm-up Draw a water molecule. Include the
  hydrogen, oxygen atom(s) for each. Write the
  charge on each atom.
• Why is it called a molecule?
• Define hydrogen bond
• polar covalent water molecule

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WATER

• Most abundant compound
• in most living things
• A molecule because it shares electrons
• Made up of weak hydrogen bonds
• easily broken
• Polar covalent - one side of the
• molecule has a slight (?), one side
• is slightly (?).

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pH scale