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periodic table trend

QuestionAnswer
Metal properties Shiny (luster) Solids at STP (except Mercury) Good conductors of Heat and Electricity (bc of highly mobile valence electrons) Malleable and Ductile
Non-metal properties Dull, at STP many are Gases, some are solids, and one is a liquid (Bromine) NM Solids are poor conductors & brittle
Diatomic elements HOFBrINCl
Chemical Metal Properties Generally lose electrons in reactions, form positively charged ions (Cations) radius of a metal ion is smaller than the radius of the neutral atom
Chemical Non-metal Properties Generall gain electrons in reactions, form negatively charged ions (Anions) the radius of a non-metal ion is larger than the radius of the neutral atom
Group 1 in the periodic table is called… Alkali metals
Alkali metal properties Easily lose one valence electron - Form ions with a +1 charge - React vigorously in water
Group 2 in the periodic table is called… Alkaline Earth Metals
Alkaline earth metal properties Easily lose two valence electrons to form ions with a +2 charge. 1 & 2 Found as stable compounds not as atoms in nature
Groups 3-12 in the periodic table are called… Transition metals
Transition metal properties Can haven multiple oxidation states
Group 17 in the periodic table is called… Halogens
Halogen properties Readily gain 1 electron, form ions with -1 charge
Group 18 in the periodic table is called… Noble (Inert) Gases
Noble gas properties Stable/non-reactive monatomic gases. “Complete valence shell” fills up 8 valence electrons (s and p sublevels) 2 valence electrons of He fill its only electron shell
How does an atom become an ion? Losing or gaining electrons
Allotropes different forms of the same element, differences in properties (ex: carbon: graphite, diamond, fullerene)
What happens when you go down a group in the periodic table? More principle energy levels, more shielding from kernel electrons
What happens as you go across a period in terms of subatomic particles? More Protons in the Nucleus. Increased Nuclear Strength. Number of Energy Levels is the Same
Ionization energy the specific amount of energy required to completely remove an electron from a gaseous atom or ion
What happens to first ionization energy as you go down a group? Less energy to remove an electron. Decrease in first ionization energy
What happens to electronegativity as you go down a group? Less attraction for electrons. Decrease in electronegativity
Electronegativity how strongly an atom pulls shared electrons toward itself in a chemical bond
What happens to atomic radius as you go across a period? Electron cloud pulled in tighter. Atomic Radius decreases
What happens to first ionization energy as you go across a period? More energy to remove an electron. First Ionization Energy increases
What happens to electronegativity as you go across a period? More attraction for electrons. Electronegativity increases
What is the most electronegative element? Fluorine
What is the least (but most reactive) electronegative element? Francium
Created by: markoii
 

 



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