Download - Organizing the Periodic Table
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Warm-up 11/21
Watch the video and describe how one scientists changed aspects of the previous theory to make a new one.
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Organizing the Periodic Table
Chemists use the properties of elements to
sort them into groups
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Warm-up 11/25
• Use the periodic table to find the following information on Fluorine.– Group #– Period– # of Valence Electrons– # of Energy Levels (shells)occupied by the
electrons in Fluorine
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Mendeleev’s Periodic Table• 1869- Russian chemist &
teacher published the first table of elements to be widely accepted
• Arranged the elements into rows in order of increasing mass so that elements with similar properties were in the same column
• Left empty spaces where undiscovered elements would fit
Eka aluminum (gallium) predicted it would be a soft metal with a low melting point and a density of 5.9 g/cm3 close match=useful table!
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12/1 Warm-up• Describe 3 pieces of information
that you can get from the periodic table about an element.
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12/2 Warm-upDetermine which of these images is a metal, nonmetal and metalloid and write the clues you used to decide.
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The Modern Periodic Table• An arrangement of elements based on a set of properties that repeat
from row to row• Elements are arranged according to atomic number• 7 rows or periods- each corresponds to a principle energy level- the
# of elements per period varies because the # of available orbitals increases from energy level to energy level
• Elements within a column or group have similar properties• Properties w/in a period change as you move across the row, the
pattern repeats as you move from one period to the next
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Periodic Law• When elements are arranged in order of
increasing atomic number, there is a periodic repetition of their physical and chemical properties
Atomic radii decreases
Electronegativity decreases
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SodiumPotassium
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Metals
• 80% of elements• Good conductors of
heat and electricity• High luster- reflect light• Solids at room
temperature• Ductile
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Nonmetals
• Show greater variation in physical properties
• Most are gases at room temp.
• Properties opposite metals– Poor conductors– Brittle
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Metalloids
• Show properties similar to metals and nonmetals depending on conditions
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Round atomic mass to the nearest whole # to get mass #
Use the atomic # to find the # or protons or electrons (in a neutral atom)
Mass #-Atomic #=neutrons
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Representative Groups• Valence electron-
electron that is in the highest occupied energy level of an atom
• Valence electrons play a key role in chemical reactions
• Properties vary across a period because the # of valence electrons increases from left to right
• Elements in a group have similar properties because they have the same # of valence electrons
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Valence Electrons• When the highest
occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react.
• Electron dot diagram- a model of an atom in which each dot represents a valence electron
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Ionic Bonds• Elements that do not
have complete sets of valence electrons tend to react.
• Some elements achieve stable electron configurations through the transfer of electrons between atoms.
• When an atom gains or loses an electrons the # of protons does not equal the # of electrons this forms an ion
• Ion- charged atom• Formation of an ion
requires energy because an electron must be removed
Anions are named by using part of the element name and the suffix -ide
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To become an ion an elements electron must escape the energy levels by gaining a required about of energy called the ionization energy.
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Formation of Ionic Bond• An ionic bond is
an attraction between a cation (metal) and an anion (nonmetal)
• A ionic compound is a compound that contains ionic bonds and the net charge must be zero
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Crystal Lattices
Ionic Compounds have high melting points, are poor conductors as
solids (good when melted or in
solution), and shatter when struck with a
hammer.
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Covalent Bonds• Nonmetals will
sometimes share electrons to achieve a full set of valence electrons
• A chemical bond in which two atoms share electrons is a covalent bond
• The attraction between the shared electrons and the protons in each nucleus hold the atoms together.
Electron dot formula
Structural Formula
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Covalent Bonds• Some atoms
share more than one pair of electrons to reach a full outer shell of electrons.
• Two pairs of electrons- double bond
• Three pairs of electrons- triple bond
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Polar Covalent Bonds• In a covalent
compound with more than one type of atom the electrons may not be shared equally
• In general, elements on the right of the periodic table and at the top of groups have a greater attraction for electrons (electronegativity)
A covalent bond in which the electrons are aren’t shared equally is a polar covalent bond
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Polar and Nonpolar Molecules
• In a polar covalent bond the atom with the greater attraction for electrons has a partial negative charge and the other atom has a partial positive charge.
• An atom can have a polar bond and not be a polar molecule.
• The type of atoms and its shape determine whether a molecule is polar or not.
Which of these are polar??
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Attraction Between Molecules
• There are forces of attraction between molecules they are not strong as ionic or covalent bonds but they are strong enough to hold molecules together in a solid or a liquid
• Attractions between polar molecules are stronger than attractions between non-polar molecules
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Metallic Bonds
• The attraction between the metal cation and the shared electrons around it
• In a metal the valence electrons are free to move among the atoms- this accounts for many of the properties of metals
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Chemical Reactions• In a chemical
reaction one or more reactants react to form one or more products
• Chemical Equations are used to represent the process of a chemical reaction.
• Reactants Product
• Mass is neither created or destroyed during a chemical reaction so the number of atoms on either side of the equation must be equal.
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Balancing Equations• In order to show that mass is
conserved during a chemical reaction the equation must be balanced.
• Equations are balanced by changing the coefficient's (the numbers in front of the formulas)
• NEVER CHANGE THE SUBSCRIPTS- THAT CHANGES THE IDENTITY OF THE REACTANT OR PRODUCT
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TYPES OF REACTIONS
• Synthesis- two or more substances react to form a single substance
• A + B AB• Balance this one
– Na + Cl2 NaCl
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Decomposition Reactions
• A reaction in which a compound breaks down into two or more simpler substances.
• AB A + B• Balance this one- H2O H2 + O2
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Single Replacement Reaction
• Reaction in which one element takes the place of another.
• A + BC B + AC• Balance this one-
Cu + AgNO3 Ag + Cu (NO3)2
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Double Replacement Reaction
• Two different compounds exchange positive ions and form two new compounds
• AB + CD AD + CB
• Try These-PB(NO3)2 + KI PBI2 + KNO3
CaCO3 + HCL CaCL2 + H2CO3
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Combustion
A substance reacts rapidly with oxygen often producing heat and light
• Balance theseCH4 + O CO2 + H20
H2 + O2 H2O