the history of your periodic table ch. 6 · dobereiner--grouped elements with similar properties in...
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The History of your Periodic Table Ch. 6.1
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The History of your Periodic Table Ch. 6.1
Dobereiner--Grouped elements with
similar properties in groups of three called triads.
-studied their atomic masses.
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The History of your Periodic Table Ch. 6.1
Dobereiner--Grouped elements with
similar properties in groups of three called triads.
-studied their atomic masses.
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The History of your Periodic Table
John Newlands--grouped elements in order of atomic
mass-Called it the Law of Octaves- 7 columns eighth element goes in
the first column- Elements in same column had the
similar properties
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The History of your Periodic Table
Dmitri Mendeleev- (father of the periodic table)-Grouped elements in order of atomic mass-Elements with similar properties were placed in
same column-HIS MOST IMPORTANT CONTRIBUTION1. He left spaces open for undiscovered elements
(big jumps in mass)2. Predicted properties in those spaces with
amazing accuracy
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The History of your Periodic Table
Henry Mosely--Grouped elements in order of atomic
number-credited with modern periodic tableCame up with Period Law-
-physical and chemical properties of elements are a periodic function of their atomic numbers
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Periodic Table
Periods-a horizontal row of elements.-Tells you the electron energy levels.
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Periodic TableGroups (families)
-a vertical column of elements.-Tells us the # of valence electrons
and the elements’ chemical properties. (A Group)
-Transition metals make B Group
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Inner Transition Metal Placement
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Ch. 6.2 Periodic Table
3 types of elements1. metals
on the left side and the center, form cations
2. nonmetalson right, form anions
3. metalloidsborder control
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Ch. 10.1 Periodic Trends
A pattern of characteristics that occur over and over again
Ex days of the weeksThere are many trends on the Periodic Table
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1. Metallic Trends
Going left to right elements become less metallicGoing Down elements become more metallic
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2.
Atomic Radii
Atomic Radii is measured by taking the distance from the nucleus to the outer energy level
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Can you tell me the trend?
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Atomic Radius
DecreasesIn
crea
ses
But Why?
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Atomic RadiiAs you go down a group you are adding an energy level, or another layer of electrons
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3.
Ionic Radii
Ions aren't the same size as the atoms they come from.Cations are smaller than the parent atomAnions are bigger than the parent atom
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Ionic Radii –
Why Cations Smaller?
By losing electrons, they also lose a whole energy level, therefore, becoming smaller in size
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Ionic Radii –
Why anions bigger?
When they gain electrons, the outermost becomes full. So less force is felt by the nucleus, the atom spreads out. (becoming stable)
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4. Ch. 10.2 Ionization Energy
The energy required to removethe most loosely held electron in the outer energy level of an atom.The less energy required, the more reactive the metal
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Ionization Energy
Increases
Dec
reas
es
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Atomic Radii
+
+
e-
e-
Needs more energy to be lost
Needs less energy to be lost
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Shielding Effect
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5. Reactivity for Metals
Reactivity increases because the atom is more willing to give away its electron and react. (Ionization energy decreased)
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6. Electronegativity/Electron Affinity
Measure of an atoms attraction for an electron.Nonmetals have high attraction for electronsThe higher the attraction the more reactive the nonmetal
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Electronegativity/Electron Affinity
Increases
Dec
reas
es
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Electronegativity
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Electronegativity/Electron Affinity
One exception- noble gasesWhy?They don’t want electrons, they are happy and full already
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7. Reactivity for nonmetals
Going UP a group for nonmetals increases their reactivityThe reason more electron affinityFluorine is the most reactive nonmetal.
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Ch. 11
Families of the Periodic Table
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Periodic Table -
Regions
Transition Metals
Alkaline Earth Metals
Alkali Metals
Metalloids
Other Metals
Non MetalsHalogens
Nobel Gases
Inner Transition Metals
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Ch. 11.1 Alkali Metals Group 1
Most reactive metals (one valence e-)Found as compounds (salts).Soft metalsGood conductors.
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Brainiac Video
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Cesium
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Alkaline-earth Metals Group 2
Similar to Alkali but less reactive because they have 2 valence electronsMostly found as compounds
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Calcium
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Ch. 11.3 Transition Metals Group 3-12
Less reactive than groups 1 and 2Strong metals (Fe, Cr, Ti, Co, Zn)Good conductors
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Transition Metals
All solids with the exception of mercuryValuable metals (Ag, Au, Pt, Cu, Ni)
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Ch. 11.3 Inner Transition Metals
Two rows at the bottomRare earth metals93 and above are manmade
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Uranium
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Metalloids (Semiconductors)
7 elements on the stepProperties of both metals and non-metals.Silicon the most familiar (computer chips)Arsenic is rat poison
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Silicon
Arsenic Exposure
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Non MetalsAre not able to conduct electricity or heat very well.Found in groups 13-18 with the exception of hydrogen.
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HYDROGEN
It is not a alkali metalIt is a gas/nonmetalA very explosive gas.It is located in group one because it has one valence electronHindenburg
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Carbon
Found as an element (coal, diamond, graphite)Found in millions of different compoundsCalled Organic Compounds
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Oxygen and Nitrogen
Oxygen is the most common element found on EarthNitrogen most common gas found in the atmosphere
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Ch. 11.2 Halogens Group 17
Highly reactiveForm salts with group 1Used to kill bacteria (Cl, F, I)Bromine the only liquid nonmetal
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Noble Gases Group 18
Stable and inert gasesDon’t form compounds.Full valence shell.Fun with He
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Xenon Bulbs
Neon
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Krypton a stable violet colored gas?
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