Gen Chemistry Ch. 1: Atomic Structure

Question 1

Proton

Answer 1

Positive charge, mass around 1 amu

Question 2

Neutron

Answer 2

No charge, mass around 1 amu

Question 3

Electron

Answer 3

Negative change, negligible mass

Question 4

Nucleus of an atom

Answer 4

Contains the protons and neutrons, electrons move around the nucleus

Question 5

Atomic number (Z)

Answer 5

Number of protons in a given element, unique identifier because elements defined by number of protons

Question 6

Mass number (A)

Answer 6

Sum of an element’s protons and neutrons, can be different within an element because of isotopes

Question 7

Atomic mass

Answer 7

Essentially equal to the mass number, the sum of an element’s protons and neutrons

Question 8

Isotopes

Answer 8

Atoms of a given element (same atomic number) that have different mass numbers, differ in number of neutrons

Question 9

Isotopes of hydrogen

Answer 9

Protium, deuterium, and tritium

Question 10

Atomic weight

Answer 10

Weighted average of the naturally occurring isotopes of an element, listed by periodic table

Question 11

Rutherford model

Answer 11

The atom has a dense, positively charged nucleus that makes up only a small fraction of the volume of the atom

Question 12

Bohr model of the atom

Answer 12

A dense, positively charged nucleus is surrounded by electrons revolving around the nucleus in orbits with distinct energy levels

Question 13

Planck model

Answer 13

The energy difference between energy levels is called a quantum

Question 14

Quanta

Answer 14

Discrete bundles of energy that are emitted as electromagnetic radiation from matter

Question 15

Quantization

Answer 15

There is not an infinite range of energy levels available to the electron; electrons can exist only at certain energy levels

Question 16

Atomic absorption spectrum

Answer 16

Unique to each element, for an electron to jump from a lower energy level to a higher one, it must absorb an amount of energy precisely equal to the energy different between the two levels

Question 17

Atomic emissions spectrum

Answer 17

Unique to each element, when electrons return from an excited state to the ground state, they emit an amount of energy that is exactly equal to the energy difference between the two levels, sometimes the EM energy emitted corresponds to a frequency in the visible light range

Question 18

Quantum mechanical model

Answer 18

Electrons do not travel in defined orbits but rather are localized in orbitals

Question 19

Orbital

Answer 19

A region of space around the nucleus defined by the probability of finding an electron in that region of space

Question 20

Heisenberg uncertainty principle

Answer 20

It is impossible to know both an electron’s position and momentum exactly at the same time

Question 21

Quantum numbers

Answer 21

Completely describe any electron in an atom

Question 22

Four quantum numbers

Answer 22

n, l, ms, ml

Question 23

Principal quantum number

Answer 23

n - described the average energy of a shell

Question 24

Azimuthal quantum number

Answer 24

l - aka angular momentum quantum number, describes the subshells within a given principal energy level (s, p, d, or f), values range from 0 to n-1, s = 0, p=1, d = 2, f =3

Question 25

Magnetic quantum number

Answer 25

ml - specifies the particular orbital within a subshell where an electron is likely to be found at a given moment in time, values from -l to l

Question 26

Spin quantum number

Answer 26

ms - indicates the spin orientation of an electron in an orbital (either +1/2 or -1/2)

Question 27

Electron configuration

Answer 27

The pattern by which subshells are filled, as well as the number of electrons within each principal energy level and sub shell, uses spectroscopic notation

Question 28

Spectroscopic notation

Answer 28

Combining the n and l values as a number and letter, respectively to designate the location of electrons

Question 29

n+1 rule

Answer 29

Determines how electrons fill the principal energy levels and subshells according to increasing energy, the lower the sum of n+l, the lower the energy, if n+l is equal than the sub shell with the lowest n value will fill first

Question 30

Hunds rule

Answer 30

Describes how electrons fill orbitals, states that subshells with multiple orbitals (p, d, and f) fill electrons so that every orbital in a subshell gets one electron before any of them gets a second

Question 31

Paramagnetic materials

Answer 31

Have unpaired electrons that align with magnetic fields, attracting the material to a magnet, causes electrons to have parallel spins

Question 32

Diamagnetic materials

Answer 32

Have all paired electrons, which cannot easily be realigned, they are repelled by magnets

Question 33

Valence electrons

Answer 33

Electrons in the outermost shell available for interaction (bonding) with other atoms, least electrostatic pull from nucleus

Question 34

Fundamental unit of charge value

Answer 34

e = 1.6 e -19 C

Question 35

Attraction between nucleus and electrons

Answer 35

Masses so small that electrostatic force of attraction is far greater than the gravitational force of attraction

Question 36

Cation

Answer 36

Positively charged atom

Question 37

Anion

Answer 37

Negatively charged atom

Question 38

Mole

Answer 38

Number of "things" equal to avogadros number

Question 39

Avogadro's number

Answer 39

Na = 6.02 E 23

Question 40

Energy of a quantum

Answer 40

Described by Planck relation, E = h*f

Question 41

Plancks constant value

Answer 41

6.626 E -34 J*s

Question 42

Bohr angular momentum equation

Answer 42

L = n*h/2/pi

Question 43

Bohr energy of an electron equation

Answer 43

E = -Rh/(n^2)

Question 44

Rydberg unit of energy value

Answer 44

Rh = 2.18 E -18 J/electron

Question 45

Ground state

Answer 45

An atom in the state of lowest energy

Question 46

Excited State

Answer 46

When at least one electron has moved to a sub shell of higher than normal energy

Question 47

Electromagnetic energy of a photon equation

Answer 47

E = h*c/lambda

Question 48

Relation between wavelength and frequency equation

Answer 48

C = 3E8 = f*lambda

Question 49

Line spectrum

Answer 49

Spectrum where each line on the emission spectrum corresponds to a specific electron transition

Question 50

Lyman series

Answer 50

Group of hydrogen emission lines corresponding to transitions from energy levels n>=2 to n=1, highest energy

Question 51

Balmer series

Answer 51

Group of hydrogen emission lines corresponding to transitions from energy levels n>=3 to n=2, includes 4 wavelengths in the visible region

Question 52

Paschen series

Answer 52

Group of hydrogen emission lines corresponding to transitions from energy levels n>=4 to n=3, highest wavelength

Question 53

Energy associated with energy change equation

Answer 53

E = h*c/lambda = -Rh*[1/ni^2 - 1/nf^2]

Question 54

Pauli exclusion principle

Answer 54

No two electrons in a given atom can possess the same set of four quantum numbers

Question 55

Maximum number of electrons within a shell equation

Answer 55

num = 2*n^2

Question 56

Maximum number of electrons within a sub shell equation

Answer 56

num = 4*l + 2

Question 57

Paired electrons

Answer 57

Electrons in the same orbital that has opposite spins

Question 58

Parallel spins

Answer 58

Electrons in different orbitals that have the same spine

Question 59

Aufbau principle

Answer 59

aka building-up principle; electrons fill from lower to energy subshells and each upswell will fill completely before electrons begin to enter the next one

Question 60

Electron configuration of cations

Answer 60

Start with neutral atom, remove electrons from the subshells with the highest n first; if multiple are tied with highest n value, remove from the highest l among them

Question 61

Electron configuration exceptions

Answer 61

Chromium and copper groups because half filled and fully filled orbitals are more stable so they will take 1 electron from the s orbitals to create either a half filled or fully filled d orbital