Unit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE

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Unit 2Chapters 5 and 6Atoms/Periodic Table/
NOMENCLATURE

• NAMING AND FORMING COMPOUNDS

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Review of Atomic Structure

• What is an atom?
• The smallest particle of an element that retains
  the properties of that element.
• What are protons?
• Positively charged particle in the nucleus of an
  atom.
• What are neutrons?
• Neutral particles in the nucleus of an atom.

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Atoms

• What are electrons?
• Negatively charged particles that orbit around
  the nucleus in certain energy levels.
• What is the nucleus?
• The center of an atom where the protons and
  neutrons are. It is what gives the atom its
  mass.
• What are energy levels (orbitals)?
• Certain areas around the nucleus where electrons
  are found moving. They exist in certain energy
  levels.

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Atoms

• What are isotopes?
• Atoms of the same element that differ by the
  number of NEUTRONS

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Define...

• Atomic Number
• the number of protons inside the nucleus of an
  atom.
• It gives that atom its identity.

• Mass Number
• the weight of the nucleus an atom.
• It is the protons and neutrons added together.
• It is measured in units called AMUs (atomic mass
  units)

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Models of Atoms

• Draw a Model of a helium-4 atom
• Draw a model of a Calcium-40 atom
• Review Questions Together

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THE PERIODIC TABLE

• AN ARRANGEMENT OF THE ELEMENTS IN ROWS AND
  COLUMNS ACCORDING TO SIMILARITIES IN THEIR
  PROPERTIES.
• THEY ARE ARRANGED ACCORDING TO INCREASING NUMBER
  OF PROTONS (ATOMIC NUMBER).

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WHAT ARE GROUPS?

• COLUMNS OF ELEMENTS AND ARE GIVEN NUMBERS AND A
  LETTER OF A OR B.
• GROUP A
• Are located in the TALL columns to either side of
  the periodic table.
• They are known as the REPRESENTATIVE elements.

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Groups Continued

• GROUP B
• Are located in the center of the periodic table.
  They are the short columns in the middle.
• They are known as the TRANSITION elements.

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WHAT ARE PERIODS?

• ARE THE ROWS IN THE PERIODIC TABLE.
• THERE ARE 7 PERIODS IN THE PERIODIC TABLE.
• NUMBER THEM ON YOUR TABLE.

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WHERE ARE THE METALS AND NONMETALS?

• DRAW A LINE ON YOUR TABLE THAT SEPARATES THE
  METALS AND NONMETALS.

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3 General Categories Have Distinguishing
Properties

• METALS HAVE HIGH LUSTER WHEN CLEAN AND A HIGH
  ELECTRICAL CONDUCTIVITY.
• NONMETALS ARE NONLUSTROUS AND ARE POOR
  CONDUCTORS.

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WHAT ARE SEMIMETALS OR METALLOIDS?

• ELEMENTS WITH THE PROPERTIES OF BOTH METALS AND
  NONMETALS.
• SHADE THE METALLOIDS ON YOUR PERIODIC TABLE.

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Naming Certain Groups

• Group 1A are known as the alkali metals.
• Group 2A are known as the alkaline earth metals
• Group 7A are known as the halogens.
• Group 8A are known as the Noble Gases, or the
  Inert Gases. (they have filled outermost energy
  levels and dont like to react)

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The Inner Transition Metals (also called the rare
earth elements.)

• Located at the bottom of the Periodic Table
  bottom 2 rows.
• The two rows are called the Lanthanide and
  Actinide Series because they are named after the
  elements that start their rows Lanthanum and
  Actinium.
• They belong to period 6 and 7 respectively.

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What category do most elements belong to?

• 80 of the elements are metals. All metals are
  solids at room temperature with one exception.
• What is it?
• Mercury, Hg, is liquid at room temperature
• Review

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NomenclatureIONS and IONIC COMPOUNDS

• ION - Charged atoms (lost or gained electrons)
• Cations - are positive ions, they have lost
  electrons
• Anions - are negative ions, they have gained
  electrons.
• Model how sodium and chlorine atoms form ions.

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Ionic Compounds Cont

• Show Magnesium atom forming magnesium ion
• Draw a compound between magnesium and chlorine

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Naming

• How do we name positive ions?
• Simply say the name of the element with the word
  ion after it.
• How do we name negative ions?
• Change the last part of the elements name to end
  with IDE
• Chlorine becomes Chloride
• Sulfur become Sulfide

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Physical Properties of IONIC COMPOUNDS

• CALLED A FORMULA UNIT.
• MADE UP OF IONS. A POSITIVE HOOKED TO A
  NEGATIVE. THEIR CHARGE MUST ADD TO ZERO.
• METAL ION () HOOKED TO NONMETAL (-).
• ARE SOLIDS AT ROOM TEMP.
• HAVE HIGH MELTING POINTS.

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Review

• Problems in notepack

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Periodic Table

• There is a pattern in predicting how many
  electrons are lost and gained for the
  REPRESENTATIVE ELEMENTS.
• Write these charges onto your periodic table with
  me now.

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MOLECULAR COMPOUNDS

• MOLECULES ARE THE SMALLEST ELECTRICALLY NEUTRAL
  UNIT OF A SUBSTANCE THAT STILL HAS THE PROPERTIES
  OF THE SUBSTANCE.
• MOLECULES ARE MADE UP OF TWO OR MORE NONMETALS
  THAT ACT AS A UNIT.

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More on Molecules

• MOLECULES ARE MADE UP OF NONMETALS SHARING
  ELECTRONS.
• This is called a COVALENT BOND
• Draw a model of a hydrogen molecule
• Water
• Carbon dioxide

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Physical Properties that Molecules Share

• THEY CAN BE A SOLID, LIQUID, OR A GAS AT ROOM
  TEMPERATURE.
• HAVE LOW MELTING POINTS.

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REVIEW!!MOLECULES VS FORMULA UNITS

• MOLECULE - A GROUP OF NEUTRAL ATOMS THAT ACT AS A
  UNIT.
• TWO OR MORE NONMETALS COVALENTLY BONDED. ELECTRON
  SHARING.
• FORMULA UNIT- COMPOSED OF A CATION WITH AN ANION.
• METAL () WITH A NONMETAL(-).
• IONIC BOND ELECTRON TRANSFER.

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CHEMICAL FORMULAS

• SHOWS THE KINDS AND NUMBERS OF ATOMS IN THE
  SMALLEST REPRESENTATIVE UNIT OF THE SUBSTANCE.
• Monatomic elements are represented by their
  Symbols.

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7 Naturally Occurring Diatomic Molecules

• There are 7 naturally occurring diatomic
  elements. Write them down and star them on your
  periodic tables...
• H2 F2
• O2 Cl2
• N2 Br2
• I2

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Formulas

• Molecular Formulas - shows the kinds and numbers
  of atoms present in a molecule of a compound.
• We cannot determine the shape or geometry.
• CO2 has 1 carbon atom and 2 oxygen atoms. We
  dont know how connected.

• Formula Units - The lowest whole number ratio of
  ions in a compound.
• Formula Units form repeating three-dimensional
  crystals.

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How can we name the ions of transition metals
(including tin and lead?

• Since these elements have more than one common
  charge, we must tell the reader how many
  electrons were lost when forming the compound.
• We use ROMAN NUMERALS to indicate how many
  electrons were lost.
• Copper (II) ion - lost two electrons
• Tin (IV) ion - lost 4 electrons