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
5 electron groups
3 bonding groups
2 lone pairs
electron: trigonal bipyramidal
molecular: t shaped
angle <90
Hybridization: sp3d
5 electron groups
2 bonding groups
3 lone pairs
electron: trigonal bipyramidal
molecular: linear
angle 180
Hybridization: sp3d
6 electron groups
6 bonding groups
0 long pairs
electron octahedral
molecular octahedral
angle 90
Hybridzation: sp3d2
6 electron groups
5bonding groups
1 lone pair
electron octahedral
molecular square pyramidal
angle <90
Hybridzation: sp3d2
6 electron groups
4 bonding groups
2 lone pairs
electron octahedral
molecular square planar
angle 90
Hybridzation: sp3d2
ClF3: polar, non polar, or ionic
polar
NH3 ionic, polar, non polar
polar
Li3N ionic, polar, nonpolar
ionic
C2H4 polar, non polar, or ionic
non polar
PCl3 polar, non polar, ionic
polar
H2O polar non polar ionic
polar
Cl4C polar, non, ionic
non polar
SF6 polar, non polar, ionic
non polar
PF5 ionic, polar, non polar,
non polar
C2H3N. polar non polar ionic
polar
XeF4 ionic, polar, non polar
non polar
which element will form the most polar bond with fluorine
Boron
N2 polar, non polar, ionic
non polar
general trends in electronegativity values
increase from left to right, decrease from top to bottom
what type of intermolecular forces are found in H2CO
dispersion and dipole-dipole forces
Wha types of intermolecular forces are found in CH2Cl2
dispersion and dipole-dipole forces
London Dispersion force (LDF)
present/possible for any atom and all covalent compounds
-polar or non polar
Dipole interactions
only exist in polar covalent molecules because required to have a permanent dipole
Hydrogen bonds
special dipole-dipole meets these conditions:
- molecule must have H in a very polar bond (H bonded to N,O,F)
- neighbor molecules must have a N,O,F (atoms with high electronegativity and lone pairs of electrons)
Dipole bonds in liquids vs solids
Liquids: attractions and repulsions
solid: only attractions
Which bonds are harder to break
those with higher boiling point and melting point, therefor a higher LDF
MW, LDF, MP, and BP, surface area, and period
MW increases LDF increases Boiling point Increases Melting point: increaeses More surface area Peroid decreases
polarizability
ability to “squash manipulate the electronic cloud
Low polaralizabeility vs high
Low= “hard” low LMF
High=”soft” high LMF
CO2 polar or nonpolar
non polar
CH4 polar or non polar
non polar
what type of interaction will occur between H2O and Na+
ion-dipole forces
C+H bonded
always non polar
same ions/atoms bonded together
always non polar
BF4 polar or non polar
non polar
energy levels of bonding and antibonding orbitals?
The energy of a bonding orbital is always lower than the energy of the corresponding antibonding orbital.
Diamagnetic vs paramagnetic
Diamagnetic: all of the electrons are paired
Paramagnetic because it has unpaired electrons
What type of orbitals overlap to form the N-H bond in NH3?
sp3 of nitrogen and s of hydrogen
formula for bond order
(electrons in bonding orbitals - electrons anti bonding orbitals)/2
bond order definition
the number of chemical bonds between a pair of atoms.
the energy of a boding orbital is…
always lower than th energy of the corresponding anti bonding orbital
valence bond theory is based on the idea that
electrons in atomic or hybrid orbitals overlap to form bonds
the higher the bond order…
the more stable the bond
how are the number of standard atomic orbitals related to he number of hybrid atomic orbitals
they are equal
what is hybridization
The mathematical combination of standard atomic orbitals to form hybrid atomic orbitals where the number of standard atomic orbitals equals the number of hybrid atomic orbitals
what orbitals overlap occur to form triple bond
one sigma bond and two pi bonds
Which of the properties of a liquid are dependent on the intermolecular attractive forces in the liquid?
viscosity, surface tension, density
