Final Flashcards
effective nuclear charge (Zeff)
- increases from left to right
- stays the same top to bottom(increases slightly)
Core size
- Decreases from left to right
- Increases as descends
Electron affinity
- more negative left to right
- more positive most positive as descends frst column only
- -no clear trend in general going down
Melting point
GROUP 1A: Decreases as descends
Group 7A: Increases as descends
Density
GROUP 1A: Decreases as descends
Group 7A: Increases as descends
Metallic Characteristics
- decreases from left to right
- Increases as descends
ionization energy
-energy needed to remove an electron
- Increases from left to right
- Decreases as descends
Halogens with respect to electron affinity
very exothermic electron affinity values
-electron affinity values are more negative for elements that prefer to gain, rather than lose, an electron (negative ions)
boiling part for group 7A
-increase as descends
what is true regarding ionization energies
they are all endothermic
Elements have a series of ionization energies for removing the first and additional electrons from the atom. Each ionization energy increases for successive electrons being removed. Where will the largest jump in ionization energies occur for aluminum?
Aluminum because it has there valence electrons so the fourth, the shell electron will be the hardest to remove
what is the most reactive nonmetal, in fairly extremes circumstances,
fluorine
The effective nuclear charge is the amount of charge experienced by an electron taking into account any shielding effects from other electrons. Electrons between the nucleus and the electron of interest cause shielding and reduce the actual charge felt by the electron of interest.
The outermost electron of boron experiences a lower effective nuclear charge than carbon. Why?
The nuclear charge increases from boron to carbon, but there is no additional shielding.
what happens as you move down he rows
Higher energy levels
-more electronic shells
what happens as you move across the columns
more electronic valence shells
how to alkali metals react with halogens
diatomic elements that reacts vigorously with sodium metal to produce compounds for example
Br2+2Na–2BrN
size comparison anion, cation, neutral
Anion, Neutral, Cation
Biggest——->Smallest
How many covalent bonds are usually formed from the element F
1
when is it appropriate to form double or triple bonds in a Less Structure?
when the central atom does not have an octet of electrons
How many covalent bonds are usually formed from the element H
1
How many covalent bonds usually formed by N
3
How many covalent bonds usually formed by O
2
How many covalent bonds are usually formed by the element C
4
2 electron groups
2 bonding groups
0 lone pairs
Electron: linear
Molecular: linear
Angles: 180
Hybridization: sp
3 electron groups
3 bonding groups
0 lone pairs
electron: trigonal planar
molecular: trigonal planar
angle: 120
Hybridization: sp2
3 electron groups
2 bonding groups
1 lone pair
electron: trigonal planar
molecular: bent
angle: <120
Hybridization: sp2
4 electron groups
4 bonding groups
0 lone pair
electron: tetrahedral
molecular: tetrahedral
angel: 109.5
Hybridization: sp3
4 electron groups
3 bonding groups
1 lone pair
electron: tetrahedral
molecular: trigonal pyramidal
angle: <109.5
Hybridization: sp3
4 electron groups
2 bonding gropus
2 lone pairs
electron: tetrahedral
molecular: bent
angle: «109.5
Hybridization: sp3
5 electron groups
5 bonding groups
0 lone pairs
electron: trigonal bipyramidal
Molecular: trigonal bipyramidal
angle 120 equatorial 90 axial
Hybridization: sp3d
5 electron groups
4 bonding groups
1 lone pair
electron trigonal bipyramidal molecular: seesaw ange: <120 equatorial <90 axial Hybridization: sp3d