periodic trends and bonding chapters 5 & 6. ions and valence electrons how many valence...
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Periodic Trends and Bonding
Chapters 5 & 6
Ions and valence electrons
How many valence electrons are in the following elements? Na Mg H He Cl Al
Show your Understanding
Draw the Lewis dot structures for each of those elements
What ions will those elements form?
S- block
Chemically reactive metals Group #1= alkali metals
Slippery appearance and can be cut with a knife! For real?
They all have one valence electron Combine readily with the halogens to form salts
Group #2- Alkaline Earth Metals Harder, denser and stronger than group #1 metals Have 2 valence electrons
d- block - Transition Metals
Lowest quantum # = 3 Maximum # of electrons = 10 There are exception to the electron
configuration rules Some metals may form several different ions They are all metals and good conductors of
heat and electricity and have high luster. Properties vary greatly.
Some metals are highly reactive Other metals not so much- Au, Pt, Pd
p-block – Groups 13-18
Group 13- 3 valence electrons Group 14 – 4 valence electrons Group 15- 5 valence electrons etc. etc. Contains metals, non-metals and metalloids. Important group- #17- Halogens
Most are gases- most reactive with metals
Main Group elements
Elements found in the s block and p block Only elements that can be used in Lewis Dot
Structures
Key Concepts/ Terms
Electrons have an attraction or pull towards the nucleus of the atom.
Shielding/ Screening: the attraction of outer shell electrons is counterbalanced by the repulsion of the inner-shell electrons. The inner-shell electrons “screen” or “shield” the outer-shell electrons from full attraction
Atomic Radii
TREND: Increases from top to bottom Decreases from left to right
Arrange the following in increasing atomic radius: Rb, In, Sb, Sr, I
Ionization Energy The energy required to remove an electron (IE2) = energy req. to remove a second electron The more electrons removed from an atom the
greater the IE TREND:
Increases from left to right Decreases from top to bottom
Exceptions: ( within the same energy level) Group 3A – lower energy than 1A and 2A bc entering p
orbital, slightly higher in energy than the s orbital for the same level
Group 6A – electrons are paired up in the p-orbital and the IE slightly dips, making it easier to remove
Ionization Energy
Arrange the following elements in order of decreasing IE. Na, Mg, Al, Si
Ionization Energy
Arrange the following elements in order of decreasing IE. Na, Mg, Al, Si
Si < Al < Mg< Na
Electron Affinity
Energy absorbed when an electron is added
TREND:
Greater Attraction for electrons from left to right ( Left to right = least negative to most negative)
Decreases from top to bottom
Electron Affinity
Which group would be the easiest to add an electron to?
Arrange the following elements in increasing electron affinity: C, Si, Ge Cl, S, P
Electron Affinity - answer
Which group would be the easiest to add an electron to? The halogens
Arrange the following elements in the most negative to least negative electron affinity: C, Si, Ge – same Cl, S, P – same
Ionic Radii- DO NOT DO
Term: Isoelectronic : species that have the same number of electrons. ( Na+, Mg2+)
TREND: Top to Bottom = increases Left to right = decreases
Ionic Radii
Arrange the following ions in order of increasing ionic radii:
Na+, Tl3+, Mg2+,
Ionic Radii - answer
Arrange the following ions in order of increasing ionic radii:
Mg2+, Na+, Tl3+,
Electronegativity
Ability for an atom to attract electrons When it is chemically combined with another
atom. Elements with high electronegativities
(nonmetals) often gain electrons to form anions.
Elements with low electronegativities (metals) often lose electrons to form cations.
Electronegativity
TREND:
Top to Bottom = decreases Left to right = increases