Section 1

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Tetrahedral pyramidal

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Cards (32)

Section 1

(32 cards)

Tetrahedral pyramidal

Front

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

Back