109.5 degrees, 3 bonding and 1 lone pair. Example NH3
Back
Trigonal bipyramidal Seesaw
Front
4 bonding and 1 lone pair. Example SF4
Back
Which following subshell does not exist 6g, 3f, 3p, 2s, 4d?
Front
3f
Back
Non-polar covalent
Front
Equally shared electron pairs
Back
Atomic Radii
Front
Decrease from left to right and increase down a group(r shape top to Buttom)
Back
Trigonal bipyramidal Linear
Front
2 bonding and 3 lone pairs. Example XeF2
Back
Trigonal Planar
Front
120 degrees, 3 bonding and 0 lone pairs. Example BF3
Back
Number of orbitals in a p subshell
Front
3
Back
How many p orbitals are in the n=4 subshell
Front
3 different kind of patterns two circles
Back
Octahedral
Front
90 and 90 degrees, 6 bonding and 0 lone pairs. Example SF6
Back
Electronegativity(attracts)
Front
Measure of attraction that an atom has for the electrons in a chemical bond. Atoms on right of table pick up electrons and hold them better
Back
Orbital with the quantum number N=3, l=2, m=-1 can be found?
Front
In 3d
Back
Tetrahedral bipyramidal
Front
90 and 120 degrees, 5 bonding and 0 lone pairs. Example PCl5
Back
Tetrahedral
Front
109.5 degrees, 4 bonding and 0 lone. Example CH4
Back
Trigonal Planar Bent or Angular
Front
120 degrees, 2 bonding and 1 lone pair. Example SO2
Back
Linear
Front
180 degrees. 2 bonding and 0 lone pairs. Example BeF3
Back
Octahedral square pyramidal
Front
5 bonding and 1 lone pair. Example IF5
Back
Liquid to Gas
Front
Vaporizing
Back
What is the total number of orbitals found in the n=4 shell?
Front
4x4=16
Back
Solid to Gas
Front
Sublimation- change to vapor when heated. Can change back to solid when cooled.
Back
Gas to Solid
Front
Decomposition- rotting or decaying
Back
Tetrahedral Bent or Angular
Front
109.5 degrees, 2 bonding and 2 lone pair. Example H20
Back
Different Subshells and the number of orbitals and max # of electrons.
Front
s-l=0 has 1 orbital and 4 max # of electrons
P-l=1 has 3 orbitals and 6 max # of electrons
D-l=2 has 5 orbitals and 10 max # of electrons
F-l=3 has 7 orbitals and 14 max # of electrons
Back
Solid to Liquid
Front
Melting
Back
Trigonal bipyramidal T Shape
Front
3 bonding and 2 lone pairs. Example ClF3
Back
Octahedral Square Planar
Front
4 bonding and 2 lone pairs.
Back
Diamagnetic
Front
Paired electrons in an orbital
Back
Polar covelent
Front
Electron pairs is unequally shared by two atoms
Back
Liquid to Solid
Front
Freezing
Back
Paramagnetic
Front
Unpaired electron
Back
L quantum number
Front
Distinguishes different shape of the orbital
Back
Gas to Liquid
Front
Condensation- to make closer together instead of freely