Unit 2 Review

Question 1

What does a mass spectrometer do?

Answer 1

Finds the relative mass of particles

Question 2

What does M/Z mean

Answer 2

Mass per charge

Question 3

What charge do most IONS have?

Answer 3

1+

Question 4

Where are the electrons in an atom?

Answer 4

In a “cloud” surrounding the nucleus

Question 5

What subatomic particles make up the nucleus?

Answer 5

Protons and neutrons

Question 6

What charge does a proton have?

Answer 6

Positive, +1

Question 7

What charge does a neutron have?

Answer 7

No charge, 0

Question 8

What charge does an electron have?

Answer 8

Negative, -1

Question 9

What does it mean for protons and electrons if an atom is neutral?

Answer 9

The number of protons is equal to the number of electrons

Question 10

How do you find the number of protons in an element’s nucleus?

Answer 10

The atomic number on the periodic table

Question 11

Where is most of the atomic mass concentrated in an atom?

Answer 11

The nucleus, the weight largely depends on the number of protons and neutrons

Question 12

What are isotopes?

Answer 12

Two or more forms of the same element with the same number of protrons but different numbers of neutrons (that causes differences in mass)

Question 13

How do you find the percentage of each element in a molecular formula?

Answer 13

Elemental analysis: multiply the atomic mass by the number of the element, then divide by the total mass of the compound

Question 13

What is particle composition?

Answer 13

Type and number of atoms per each particle

Question 14

How do you find molar mass on a spectrum?

Answer 14

Look to the peak furthest on the right, and its number on the x-axis is the molar mass

Question 15

What is the relationship of frequency to wavelength?

Answer 15

frequency= (constant)/(wavelength)

Question 16

What is plank’s constant or (h)?

Answer 16

6.626 * 10^-34 j/s

Question 17

What is visible light and its range?

Answer 17

400-700nm, it is light that can be seen by human eye, medium length wavelengths

Question 18

How to find a molar photon?

Answer 18

Multiply the joules equation by avogadro’s number (then divide by 1000 for kilojoules)

Question 18

What is ultraviolet light, XRay, and Gamma ray and their range?

Answer 18

Less than 400nm, it is light that cannot be seen by humans, very small wavelengths (gamma ray is the smallest)

Question 19

What is infrared radiation?

Answer 19

Medium large waves, the range is 700nm-1m

Question 20

The higher the energy, the what the wavelength?

Answer 20

Shorter

Question 21

The lower the energy, the what the wavelength?

Answer 21

Longer

Question 22

What are microwaves?

Answer 22

Medium large waves (bigger than infrared) and their range is >1m

Question 23

Can any substance absorb all types of wavelengths?

Answer 23

No, any substance only has a set amount of wavelengths they can absorb (bc energy is not continuous)

Question 24

Can electrons orbit in the space between rings?

Answer 24

NO

Question 25

What is an atom's ground state?

Answer 25

The lowest energy state, where the electron is on the ring CLOSEST to the nucleus

Question 26

What is an atom's excited state?

Answer 26

The highest energy state, where the electron is on ANY OTHER RING THAN THE FIRST from the nucleus

Question 27

The longer the wavelength, the less the energy, so the electron will...

Answer 27

NOT jump to as far of an orbit

Question 28

What is absorption?

Answer 28

When energy is absorbed by an atom and the electron jumps from the ground state to a higher energy orbit

Question 29

What happens to potential, kinetic, and total energy during absorption?

Answer 29

PE increases (more energy=less IMFS), KE decreases (due to space between electrons), and total energy increases (PE>KE)

Question 30

What is emission?

Answer 30

When an atom releases energy (in the form of a photon that corresponds to the energy gap between orbits) and the electron comes down from a higher energy orbit to a lower one

Question 31

What happens to potential, kinetic, and total energy when emission happens?

Answer 31

PE decreases, KE increases, and total energy decreases

Question 32

What holds atoms together in a bond?

Answer 32

Electrons

Question 32

What happens when electrons interact with visible/UV light?

Answer 32

The bonds break (also known as an electronic transition)

Question 33

If infrared (less than visible light) has lower energy than visible light, what transition does it do?

Answer 33

Vibrational transitions

Question 34

If microwaves have less energy than infrared, what transition does it do?

Answer 34

Rotational, for it requires the least amount of energy and has the longest wavelength

Question 34

What is a covalent bond?

Answer 34

The balanced sharing of electrons between nonmetals, and the nuclei are not touching

Question 35

What is a covalent bonding model?

Answer 35

atoms are assumed to be bonded or connected to each other in molecular compounds

Question 36

What is the delocalization of electrons and how does it happen?

Answer 36

When electrons are not associated with an atom or a covalent bond, this happens when the nuclei of two atoms get too close to each other

Question 36

What happens to the potential, kinetic, and total energy during delocalization?

Answer 36

PE decreases (more space for electrons to move), KE decreases (more space means less friction), and TE decreases

Question 37

What happens to energy and stability of an atom during bond formation?

Answer 37

Bond formation releases energy, which then stabilizes the atom

Question 38

How do you find the number of neutrons in an isotope?

Answer 38

Subtract the atomic number by the mass number

Question 39

What is the speed of light?

Answer 39

450nm, or 6.67 * 10^14 hz

Question 40

What spectrum of light tells how many bonds are in a molecule?

Answer 40

Infrared

Question 41

Is vibration frequency the same in any bond?

Answer 41

NO, vibrational frequency is different in each bond

Question 42

What determines the size of an atom?

Answer 42

The electron cloud size

Question 43

What is the attractive relationship between protons and electrons in an atom?

Answer 43

The more protons there are in an atom, the more attracted electrons are to the nucleus

Question 44

What is the relationship between an electron cloud size and the number of protons?

Answer 44

The larger the number of protons, the smaller the electron cloud