Ch. 1: Atomic Structure

Question 1

Proton

Answer 1

Positive charge and mass around 1 amu; charge of fundamental unit of charge (e= 1.6*10^-19 C)

Question 2

Neutron

Answer 2

No charge and mass around 1 amu, mass only slightly larger than proton

Question 3

Electron

Answer 3

Negative charge (equal magnitude of proton) and negligible mass

Question 4

Nucleus

Answer 4

Contains the protons and neutrons, while the electrons move around the nucleus

Question 5

Atomic Number

Answer 5

Number of protons in a given element, unique identifier for each element

Question 6

Mass Number

Answer 6

Sum of an element’s protons and neutrons

Question 7

Cation

Answer 7

Positively charged atom

Question 8

Anion

Answer 8

negatively charged atom

Question 9

Atomic mass

Answer 9

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

Question 10

Isotopes

Answer 10

Atoms of a given element (same atomic number) that have different mass numbers. Differ in the number of neutrons

Question 11

Isotope Identification

Answer 11

The element followed by the mass number (ex: carbon-12, carbon-13)

Question 12

3 Isotopes of Hydrogen

Answer 12

Protium, deuterium, and tritium

Question 13

Atomic Weight

Answer 13

Weighted average of the naturally occurring isotopes of an element. The periodic table lists atomic weights, not atomic masses

Question 14

Rutherford

Answer 14

Postulated that the atom had a dense, positively charged nucleus that made up only a small fraction of the volume of the atom with gold foil experiment

Question 15

Bohr Model of the Atom

Answer 15

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

Question 16

Quantum

Answer 16

Energy diff between energy levels, first described by Planck

Question 17

Quantization

Answer 17

There is not an infinite range of energy levels available to an electron; electrons can exist only at certain energy levels. The energy of an electron increases the farther it is from the nucleus

Question 18

Planck relation

Answer 18

E=hf; E is the energy of a quantum, h is planck’s constant, and f is frequency of radiation

Question 19

Atomic Absorption Spectrum

Answer 19

Unique; 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 difference between the two levels

Question 20

Atomic Emission Spectrum

Answer 20

When electrons return from the excited state to the ground state, they emit an amound of energy that is exactly equal to the energy diff between the two levels; every element has a characteristic atomic emission spectrum and sometimes the electromagnetic energy emitted corresponds to a frequency in the visible light range

Question 21

Quantum Mechanical Model

Answer 21

Posits that electrons do not travel in defined orbits but rather are localized in orbitals

Question 22

Orbital

Answer 22

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

Question 23

Heisenberg Uncertainty Principle

Answer 23

States that it is impossible to know both an electron’s position and its momentum exactly at the same time

Question 24

Quantum numbers:

Answer 24

4, completely describe any electron in an atom; according to pauli exclusion principle no 2 electrons in a given atom can possess the same set of 4 quantum numbers

Question 25

Principle Quantum Number

Answer 25

n, describes the averege energy of a shell; energy diff from one shell to the next is a function of (1/ni^2)-(1/nf^2)

Question 26

Azimuthal Quantum Number

Answer 26

l, describes the subshells within a given principle energy level (s, p, d, f)– spectroscopic notation refers to 1s^2 2s^2 sp^6 etc notation

Question 27

Magnetic Quantum Number ml

Answer 27

Specifies the particular orbital within a subshel where an electron is likely to be found at a given moment in time (-l to +l)

Question 28

Spin Quantum Number (ms)

Answer 28

Indicates the spin orientation (+ or - ½) of an electron in an orbital

Question 29

Electron Configuration

Answer 29

Uses spectroscopic notation (combining the n and l values as a number and letter, respectively) to designate the location of electrons

Question 30

n+l Rule

Answer 30

Electrons fill the principle energy levels and subshells according to increasing energy , which can be determined by the n+l rule

Question 31

Hund’s Rule

Answer 31

electrons fill orbitals according to Hund’s rule, which states that subshells w 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 32

Paramagnetic

Answer 32

Have unpaired electrons that align with magnetic fields, attracting the material to a magnet

Question 33

Diamagnetic

Answer 33

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

Question 34

Valence Electrons:

Answer 34

Those electrons in the outermost shell available for interaction (bonding) with other atoms

Question 35

Representative Element VEs

Answer 35

Groups 1, 2, and 13-18, the valence electrons are found in s- and/or p-orbitals

Question 36

Transition elements

Answer 36

Valence electrons are found in s- and either d- or f- orbitals

Question 37

Octet Rule

Answer 37

Many atoms interact with other atoms to form bonds that complete an octet in the valence shell