Transcript Electron Energy Levels - Winona Independent School District

Electron Energy Levels
Transition Metals electrons
• 21 -30 Transition Metals
Symbol
Electrons per energy level
Sc
2-8-9-2
Ti
2-8-10-2
V
2-8-11-2
Cr
2-8-13-1*
Mn
2-8-13-2
Fe
2-8-14-2
Co
2-8-15-2
Ni
2-8-16-2
Cu
2-8-18-1*
Zn
2-8-18-2
Valence Electrons
• The number of electrons in the outer
energy level of an atom.
If the outer energy levels are full the atom is
stable (will not combine with other atoms)
If the outer energy levels are not full, then
these atom will react (join) with other
atoms by gaining, losing or sharing
electrons to form new substances. These
types of atoms are reactive.
Guess the Valence
1
4
8
NOTE: ATOMS WANT TO FILL THEIR OUTER
LEVELS
• Atoms on the LEFT hand side of the periodic
table are more likely to LOOSE
ELECTRONS
• Atoms on the RIGHT hand side of the
periodic table are more likely to GAIN
ELECTRONS
Alkali Metals – Group 1
• Most Reactive of the Metals.
• Because they only 1 electron in the outer
energy level
1
So their valence is _______
Characteristics; soft, silver, shiny, low density
Sodium
http://www.ptable.com/
Alkali Metals – Group 1
***Please note: Hydrogen is NOT a metal is a
GAS.
It is in the first column (family) because it has
1 electron in its outer level and its very
reactive.
Hydrogen’s physical properties are more like
NONMETALS, because it’s a GAS.
Alkaline – Earth Metals Group 2
• Not as reactive as group 1, because they
have 2 electrons in its outer energy level.
2
So its valence is _______
Characteristics: silver, more dense than
alkali metals
Transition Metals Groups 3-12
• less reactive than the first 2 groups.
• They don’t lose their electrons very easily.
• Most of the transition metals have a valence of
2
• To keep the chart from being to wide, 2 rows Periods 6 & 7
taken out and added to the bottom:
- Lanthanides are shiny, reactive metals that make
steel.
Copper
- Actinides are radioactive and unstable.
Ex Americium is used in smoke detectors.
Metalloids Group 13 – 16
• This group has properties of both metals and
nonmetals.
***To calculate the valence for this group subtract the number
10 from the group number. Ex. 13-10= 3
All of group 13 has a valence of 3.
Most metalloids have about a ½ complete set of electrons in
their out energy level.
There are 4 subgroups to the metalloids:
1. Boron Group
2. Carbon Group
Silicon
3. Nitrogen Group
4. Oxygen Group
**the group names come from the 1st element in the family.
Nonmetals Group 17 & 18
• Nonmetals are the halogens and noble gases.
***To calculate the valence for this group subtract the
number 10 from the group number. Ex. 18 -10= 8
(exception is He which has a valence of 2)
• Group 17 is more reactive than Group 18,
because 18’s outer energy level is full and it
can’t take on or give up any electrons.
Group 17
Halogens – very reactive gas, because the
want to gain only one valence electron in
order to have a full energy level.
Characteristics – poor conductor of electricity,
reacts violently with alkali’s to form salt,
never found uncombined in nature.
Group 18
Noble Gases
This group is nonreactive because the
atoms outer energy level is filled.
They don’t combine with other elements
Neon