Dat General Chemistry Chapter 1

Front 1

What does Z in an element represent?

Back 1

Atomic number, equal to number of protons in an atom. (Top number)

Front 2

What does A in an element represent?

Back 2

Mass number, equal to number of protons and neutrons. (Bottom number)

Front 3

What are electrons farthest from the nucleus called?

Back 3

valence electrons.

Front 4

What determines the reactivity of an atom?

Back 4

valence electrons

Front 5

How are atomic masses expressed?

Back 5

AMU. 1 AMU is exactly 1/12 of the mass of Carbon-12

Front 6

What are the two measurments an atom can be weighted?

Back 6

- Atomic mass (amu)
- Atomic Weight (g/mole) (more conventional)

Front 7

What is avogadro's number?

Back 7

6.022 * 10^23

(it is the number of atoms or molecules in one mole)

Front 8

How do you find the atomic weight of an element when you are given multiple isotopes and their atomic masses?

Back 8

1.) multiply the masses of each isotope by the decimal of the percent (60% = .6)
2.) Sum all the multiplications together to give atomic weight of the element

See page 189.

Front 9

What did Ernest Rutherford discover?

Back 9

Showed an atom has a dense postively charged nucleus that only accounts for a small portion of the VOLUME of an atom.

Front 10

What did Max Planck discover?

Back 10

Developed first quantum theory, energy emitted as electromagnetic radiation from matter comes in discrete bundles called quanta.

Front 11

What is quanta?

Back 11

bundles of energy emitted as electromagnetic radiation from matter.

Front 12

What is the equation to find the energy value of quantum?

Back 12

E = hf

h = planck's constant = 6.626 * 10^-34 J*S

f = frequency of radiation

Front 13

What is planck's constant?

Back 13

6.626 * 10^-34 J*S

Represents H in the quantum equation
E=hf

f= frequency

Front 14

What is the equation for angular momentum?

Back 14

angular momentum = nh/2(pie)

h=planck's constant
n=quantum number (any positive integer)

Front 15

What is the only value in the angular momentum equation that can change total angular momentum?

Back 15

n (which equals quantum number)

(the energy of the electron changes in discrete amounts only with respect to the quantum number)

Front 16

The energy of the electron changes in discrete amounts only with respect to the __________________.

Back 16

Quantum number (n) (pg 190)

Front 17

The energy of an electron is ________.

Back 17

Quantized. (pg 190)

Front 18

The smaller the orbital radius, the _______ the energy state of the electrion?

Back 18

lower

Front 19

The larger the orbital radius, the _______ the energy state of the electrion?

Back 19

higher

Front 20

What is the term to describe when when electrons are excited and they release photons when returning to their ground state.

Back 20

Atomic emission Spectra

(E=hc/lambda)

Front 21

What does Atomic emission spectra provide?

Back 21

The electromagnetic energy of photons that are released as an excited electron returns to its ground state.

(E=hc/lambda)

Front 22

What is the equation for the atomic emission spectra?

Back 22

(E=hc/lambda)

h= planck's constant
c = velocity of light (3.00*10^8 m/s)
lamda = the wavelength of the radiation

Front 23

What is atomic emission spectrum?

Back 23

Quantized energies of light do not produce a continuous spectrum. This spectrum is composed of light at specific frequencies. Each line on the spectrum corresponds to a specific electronic transition. (pg 191)

Front 24

Do different elements have different atomic emission spectrums? Explain.

Back 24

Yes. Each element has each electron exicited to different energy levels, creates a fingerprint of the element.

(pg 191)

Front 25

What is the Balmer Series?

Back 25

Hydrogen emission lines corresponding to transitions from upper levels n>2 to n=2. (pg 191)

Front 26

What is the Lyman Series?

Back 26

Hydrogen emission lines corresponding to transitions from upper leves n>1 to n=1. (pg 191)

Front 27

What is the atomic absorption spectra

Back 27

The amount of energy needed to be absorbed by an electron to jump from an orbital of low energy to one of higher energy.

Front 28

What is the main difference in the Quantum mechanical model and bohrs model that was corrected?

Back 28

Electrons are now described as being in a state of rapid motion within regions of space around the nucleus called orbitals.

Front 29

What is the Heisenberg Uncertainty Principle?

Back 29

pinpointing the exact position and momentum is impossible.

Front 30

What are the four quantum numbers?

Back 30

-N (Principle quantum number) (shell)
-l (Azimuthal quantum number) (subshell)
-ml (Magnetic quantum number)
-ms (Spin quantum number)

Front 31

What is the pauli exclusion principle?

Back 31

no two electrons in a given atom can posses the same set of four quantum numbers.

Front 32

The larger the integer of the principle quantum number, the _______ the energy level.

Back 32

higher

Front 33

What is the maximum number of electrons in each principle quantum number, (n) or (shell)?

Back 33

2n^2

Front 34

The difference between the 3rd and 4th shell is __________ than that between the 2nd and 3rd shells?

Back 34

less.

Front 35

What is the value of the azimuthal quantum number or (angular momentum number)?

Back 35

any integer in the range of 0 to n-1.

The four subshells corresponding to l=0,1,2, and 3 are known as s,p,d,f.

Front 36

What are the subshells in order according the the azimuthal quantum number?

Back 36

s=0, p=1, d=2, and f=3

Front 37

What is the maximum number of electrons that can exist within a subshell?

Back 37

4*(azimuthal number) +2

(Pg 193)

Front 38

A greater azimuthal number means the _________ the energy of the subshell

Back 38

greater

Front 39

The 4s subshell will have a _______ energy than the 3d subshell.

Explain.

Back 39

-lower.

- because its average distance from the nucleus is smaller.

Front 40

What does the magnetic quantum number specify?

Back 40

The particular orbital within a subshell where an electron is likely to be found?

Front 41

How do you determine the value for the magnetic quantum number?

Back 41

Integers from L to -L, including 0.

Front 42

How many orbitals will the p subshell contain?

Back 42

3 orbitals

p --> L = 1
ml or magnetic quantum number = -1,0,1 = (3 orbitals)

Front 43

How many orbitals with the f subshell contain?

Back 43

7 orbitals

f --> L = 3
ml or magnetic quantum number = -3, -2,-1,0,1,2,3 = (7 orbitals)

Front 44

What is parallel spin?

Back 44

Electrons in DIFFERENT orbitals with the same Spin quantum number.

Front 45

How do you determine the order subshells are filled?

Back 45

n+L rule.

Front 46

Which will fill first, the 3d or the 4s subshell?

Back 46

-4s


3d --> n=3 + L = 2 ---> 5
4s ---> n=4 + L = 0 ---> 4
4s fills faster.

Front 47

To determine which subshells are filled, if an atom has a positive 1 charge, what would you do?

Back 47

1.) Determine number of electrons based on atomic number
2.) Subtract 1, because it is positive 1 charge.

Front 48

What is Hund's rule?

Back 48

Within a subshell, orbitals are filled such that there are a maxium number of half-filled orbitals with parallel spins.

Front 49

What is a paramagnetic atom?

Back 49

An element with unpaired electrons, aligns with magnetic field according to spins of these electrons.

Front 50

What is a diamagnetic atom?

Back 50

An element with no unpaired electrons and repelled by a magnetic field.