Mid-Term 1 CH231H

Question 1

How is the atomic mass calculated?

Answer 1

(weight of isotope x abundance)+(weight of isotope x abundance)

Question 2

What is an isotope?

Answer 2

A version of a singular element with different numbers of neutrons.

Question 3

What is an Ion?

Answer 3

A version of an element with different numbers of protons. (Alters the charge)

Question 4

1 mole

Answer 4

A way of measuring 6.022x10^23 units
(The number of atoms in 12g of carbon-12.)

Question 5

When frequency increases, wavelength________.

Answer 5

Decreases

Question 6

When wavelength decreases, energy______.

Answer 6

Increses

Question 7

When frequency decreases, wavelength________.

Answer 7

Increses

Question 8

When frequency increases, energy_____.

Answer 8

Increases

Question 9

Constructive waves ________

Answer 9

Increase amplitude (add together)

Question 10

Destructive wave interference_______

Answer 10

decrease amplitude (cancel out)

Question 11

Light can behave as both a _________, and _________.

Answer 11

Wave and particle

Question 12

How is KE of an admitted electron calculated?

Answer 12

KE=hv-(threshold frequency)

Question 13

What is threshold frequency?

Answer 13

The frequency of a wave needed for an electron to be released from a surface.
(hv)

Question 14

Releasing an electron requires a certain
1) wavelength/frequency
2) amplitude
3) velocity

Answer 14

Wavelength or frequency.

Question 15

Which orbital has the highest energy?

Answer 15

f-orbital (At least for the standard orbitals)

Question 16

What does the uncertainty principle tell us?

Answer 16

It tells us the uncertainty of the position of the electron.

Question 17

what does QN n tell us?

Answer 17

1)The size and energy of orbital nodes.
(written in all positive integers)

Question 18

What does QN l tell us?

Answer 18

2)The shape of an orbital
(n-1)

Question 19

What does QN Ml tell us?

Answer 19

3) Overall orientation
(Any integer between -l and l)

Question 20

What does Ms tell us?

Answer 20

4)Value of the electron
(-1/2 or 1/2)

Question 21

How many types of S-orbitals?

Answer 21

1 (2 possible electrons)

Question 22

How many types of P-orbitals?

Answer 22

3 (6 possible electrons)

Question 23

How many types of D-orbitals?

Answer 23

5 (10 possible electrons)

Question 24

How many types of F-orbitals?

Answer 24

7 (14 possible electrons)

Question 25

Electrons _________ energy going down in ring levels.

Answer 25

Give off

Question 26

Values for each letter of l

Answer 26

S=0 P=1 D=2 F=3 (its n-1)

Question 27

Electrons fill the ________ energy levels first.

Answer 27

Lowest

Question 28

Electrons don’t fill the orbital until________.

Answer 28

Every orbital has at least one electron.

Question 29

What is significant about the farthest right column of the periodic table?

Answer 29

These don’t have any valence electrons.

Question 30

Valence electron

Answer 30

Electrons that aren’t in a full shell. (A non core electron)

Question 31

Core electron

Answer 31

Electrons that are part of a full shell (A non valence electron)

Question 32

What determines which ion of an element is most common?

Answer 32

Atoms strive to be stable. This means they seek out electrons that will fill their shell fully or seek to get rid of awkwardly lingering electrons.

Question 33

In what column of the periodic table do naturally occurring ions go from being a positive ion to negative ion?

Answer 33

5A (15) This is because these non-metals like to gain extra electrons as opposed to giving off a large number of electrons.

Question 34

What is a paramagnetic electron?

Answer 34

An ion of an atom with a partially filled n-orbital.
(ex. 2s^2, 2p^4 is paramagnetic because the p-orbital isn’t filled)

Question 35

What is a diamagnetic electron?

Answer 35

An ion of an atom with a fully filled n-orbital.
(ex. 2s^2, 2p^6 is diamagnetic because the p-orbital is fully filled)