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Flashcards in Unit 1 Deck (14)
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1

Where is the probability of finding an electron in S orbitals?

The probability is highest near the nucleus and decreases as we move outward

2

Where is the probability of finding electrons in P orbitals?

There is equal probability of finding electrons in either lobe but is 0 in the nodal plane

3

What does the Aufbau principle state?

Lowest energy orbitals are filled first

4

What does Pauli’s exclusion principle state?

Only two electrons can occupy and orbital and they must have opposite spins

5

What is Hund’s rule?

If two or more empty orbitals of equal energy are available, one electron occupies each with their spins parallel until all are half filled

6

Where are expanded Octets common?

For elements in the third row and beyond

7

How does electronegative increase?

As you move up and to the right of the periodic table

8

What is a bond dipole?

The difference in electronegativity between atoms of a bond

9

What are Sigma bonds?

Bonds that form between 2 hybrid orbitals

10

Why kind of bonding results in a sigma bond?

Head on bonding

11

What kind of bonding results in a pi bond?

Indirect site by side bonding

12

What kind of bond is stronger?

Sigma bonds on stronger because there is more orbital overlap making them more stable and less reactive

13

What do electrons in a bonding orbital do?

Stabilize a molecule

14

What do electrons in an anti bonding orbital do?

Destabilize a molecule