Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
50 Cards in this Set
- Front
- Back
What does Z in an element represent?
|
Atomic number, equal to number of protons in an atom. (Top number)
|
|
What does A in an element represent?
|
Mass number, equal to number of protons and neutrons. (Bottom number)
|
|
What are electrons farthest from the nucleus called?
|
valence electrons.
|
|
What determines the reactivity of an atom?
|
valence electrons
|
|
How are atomic masses expressed?
|
AMU. 1 AMU is exactly 1/12 of the mass of Carbon-12
|
|
What are the two measurments an atom can be weighted?
|
- Atomic mass (amu)
- Atomic Weight (g/mole) (more conventional) |
|
What is avogadro's number?
|
6.022 * 10^23
(it is the number of atoms or molecules in one mole) |
|
How do you find the atomic weight of an element when you are given multiple isotopes and their atomic masses?
|
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. |
|
What did Ernest Rutherford discover?
|
Showed an atom has a dense postively charged nucleus that only accounts for a small portion of the VOLUME of an atom.
|
|
What did Max Planck discover?
|
Developed first quantum theory, energy emitted as electromagnetic radiation from matter comes in discrete bundles called quanta.
|
|
What is quanta?
|
bundles of energy emitted as electromagnetic radiation from matter.
|
|
What is the equation to find the energy value of quantum?
|
E = hf
h = planck's constant = 6.626 * 10^-34 J*S f = frequency of radiation |
|
What is planck's constant?
|
6.626 * 10^-34 J*S
Represents H in the quantum equation E=hf f= frequency |
|
What is the equation for angular momentum?
|
angular momentum = nh/2(pie)
h=planck's constant n=quantum number (any positive integer) |
|
What is the only value in the angular momentum equation that can change total angular momentum?
|
n (which equals quantum number)
(the energy of the electron changes in discrete amounts only with respect to the quantum number) |
|
The energy of the electron changes in discrete amounts only with respect to the __________________.
|
Quantum number (n) (pg 190)
|
|
The energy of an electron is ________.
|
Quantized. (pg 190)
|
|
The smaller the orbital radius, the _______ the energy state of the electrion?
|
lower
|
|
The larger the orbital radius, the _______ the energy state of the electrion?
|
higher
|
|
What is the term to describe when when electrons are excited and they release photons when returning to their ground state.
|
Atomic emission Spectra
(E=hc/lambda) |
|
What does Atomic emission spectra provide?
|
The electromagnetic energy of photons that are released as an excited electron returns to its ground state.
(E=hc/lambda) |
|
What is the equation for the atomic emission spectra?
|
(E=hc/lambda)
h= planck's constant c = velocity of light (3.00*10^8 m/s) lamda = the wavelength of the radiation |
|
What is atomic emission spectrum?
|
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)
|
|
Do different elements have different atomic emission spectrums? Explain.
|
Yes. Each element has each electron exicited to different energy levels, creates a fingerprint of the element.
(pg 191) |
|
What is the Balmer Series?
|
Hydrogen emission lines corresponding to transitions from upper levels n>2 to n=2. (pg 191)
|
|
What is the Lyman Series?
|
Hydrogen emission lines corresponding to transitions from upper leves n>1 to n=1. (pg 191)
|
|
What is the atomic absorption spectra
|
The amount of energy needed to be absorbed by an electron to jump from an orbital of low energy to one of higher energy.
|
|
What is the main difference in the Quantum mechanical model and bohrs model that was corrected?
|
Electrons are now described as being in a state of rapid motion within regions of space around the nucleus called orbitals.
|
|
What is the Heisenberg Uncertainty Principle?
|
pinpointing the exact position and momentum is impossible.
|
|
What are the four quantum numbers?
|
-N (Principle quantum number) (shell)
-l (Azimuthal quantum number) (subshell) -ml (Magnetic quantum number) -ms (Spin quantum number) |
|
What is the pauli exclusion principle?
|
no two electrons in a given atom can posses the same set of four quantum numbers.
|
|
The larger the integer of the principle quantum number, the _______ the energy level.
|
higher
|
|
What is the maximum number of electrons in each principle quantum number, (n) or (shell)?
|
2n^2
|
|
The difference between the 3rd and 4th shell is __________ than that between the 2nd and 3rd shells?
|
less.
|
|
What is the value of the azimuthal quantum number or (angular momentum number)?
|
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. |
|
What are the subshells in order according the the azimuthal quantum number?
|
s=0, p=1, d=2, and f=3
|
|
What is the maximum number of electrons that can exist within a subshell?
|
4*(azimuthal number) +2
(Pg 193) |
|
A greater azimuthal number means the _________ the energy of the subshell
|
greater
|
|
The 4s subshell will have a _______ energy than the 3d subshell.
Explain. |
-lower.
- because its average distance from the nucleus is smaller. |
|
What does the magnetic quantum number specify?
|
The particular orbital within a subshell where an electron is likely to be found?
|
|
How do you determine the value for the magnetic quantum number?
|
Integers from L to -L, including 0.
|
|
How many orbitals will the p subshell contain?
|
3 orbitals
p --> L = 1 ml or magnetic quantum number = -1,0,1 = (3 orbitals) |
|
How many orbitals with the f subshell contain?
|
7 orbitals
f --> L = 3 ml or magnetic quantum number = -3, -2,-1,0,1,2,3 = (7 orbitals) |
|
What is parallel spin?
|
Electrons in DIFFERENT orbitals with the same Spin quantum number.
|
|
How do you determine the order subshells are filled?
|
n+L rule.
|
|
Which will fill first, the 3d or the 4s subshell?
|
-4s
3d --> n=3 + L = 2 ---> 5 4s ---> n=4 + L = 0 ---> 4 4s fills faster. |
|
To determine which subshells are filled, if an atom has a positive 1 charge, what would you do?
|
1.) Determine number of electrons based on atomic number
2.) Subtract 1, because it is positive 1 charge. |
|
What is Hund's rule?
|
Within a subshell, orbitals are filled such that there are a maxium number of half-filled orbitals with parallel spins.
|
|
What is a paramagnetic atom?
|
An element with unpaired electrons, aligns with magnetic field according to spins of these electrons.
|
|
What is a diamagnetic atom?
|
An element with no unpaired electrons and repelled by a magnetic field.
|