Periodic table trends power point presentation
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Transcript of Periodic table trends power point presentation
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Periodic Table
of Elements
Cha
pter
6 N
otes
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Modern Periodic Ta
ble
Designed by Demitri Mendeleev based on atomic mass (1869)
Modified by Henry Moseley based on atomic number (1926)
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Classifying Elements
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Properties of Metals & NonmetalsMetals
•Conduct heat & electricity•Malleable•Solid at room temp (except Hg)•High luster/sheen
Nonmetals•Poor conductors•Brittle•Most are gases at room temp•Solids (sulfur & phosphorus) are dull
Gold Bromine Gas
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sToP & tHinK – metal or nonmetal
1. A gaseous substance that partially conducts electricity.
2. Solid that is malleable and shiny.3. Solid that is brittle and dull color.4. Solid that conducts electrical current and
has high luster.5. Has 7 valence electrons6. Found on the right of the ‘staircase’7. Has 1 valence electron8. d and f block elements
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Elements in the same group have similar properties! (Periodic Law)
◦ Group 1 - Alkali Metals◦ Group 2 - Alkaline Earth Metals◦ d block - Transition Metals◦ f block - Inner Transition Metals◦ Group 7 - Halogens◦ Group 8 - Noble Gases
Reactivity increases from top to bottom for 1A, 2A Reactivity decreases from top to bottom for 7A
Classifying Elements – Let’s Look at the Periodic Chart
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State the name of the group / family for each:◦ Magnesium◦ Bromine◦ Argon◦ Has 8 valence electrons◦ Group 1A◦ Copper◦ Tend to lose one electron to be more stable
(remember octet rule).
sToP & tHinK
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A groups - representative elements (s and p blocks, except noble gases)◦ Display varied properties by column
B groups - transition elements & inner transition elements (d and f blocks)◦ Fairly similar properties
A Groups & B Groups
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Atomic Radius
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Decreases across the period (row/horizontal)
Increases down the group (column/vertical)
WHY?!? – 2 Reasons
1. Each added proton increases the positive
nuclear charge… as electrons are added to
principal energy levels the level gets smaller.
2. Electrons added to a new principal energy
level are ‘shielded’ from the positive nucleus
by the electrons in lower levels.
Let’s Look @ Atomic
Radius
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1. Why does atomic radius decrease as you move from left to right on the PT?
2. Why does atomic radius increase as you move down each group on the PT?
SToP & THinK
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Anions (- charged) larger than neutral atom of the same element
Anions Ionic Radius
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Cation (+ charged) smaller than neutral atom of the same element
Cations Ionic Radius
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1. Which has a larger radius for each: ◦ K or K+? ◦ S or S2-?
2. Explain why.
SToP & THiNk
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The amount of energy required to remove an electron from an atom.
Increases up the periodic chart and from left to right.
Ionization
Energy(IE)
Trends
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Ionization Energy
(IE)Trends
(IE)
Incre
ases U
p t
he P
eri
od
ic
Ch
art
.
(IE) Increases from Left to Right
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The ability of an atom to pull electrons in a chemical bond.
Due to pull from protons and how close electrons are to nucleus.
More electronegative = stronger pull on electrons
Same pattern as ionization energy (IE)
ElectronegativityTrends
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Which is more electronegative?◦ Ca or Cl◦ P or O
In your own words, explain why ionization energy and electronegativity follow the same trend pattern on the periodic table.
SToP & THiNk