Unit 1: Atomic Structure and Properties

Question 1

Anions

Answer 1

are larger than atoms because the atom has an overall negative charge, increasing the amount of electron- electron repulsions.

Question 2

photoelectron spectrum

Answer 2

A(n) (PES) is a graph of the ionization energies for all electrons when ejected from the nucleus.

Question 3

Electrons

Answer 3

have significantly less mass than protons and neutrons and do not contribute to the mass.

Question 4

Electronegativity

Answer 4

is how much an elements nucleus attracts electrons.

Question 5

Isotopes

Answer 5

are atoms of an element with different numbers of neutrons, but same amount of protons.

Question 6

Molarity

Answer 6

(M) expresses the concentration of a solution in terms of volume.

Question 7

Percent composition

Answer 7

is the percent by mass of each element in a compound.

Question 8

Aufbau principle

Answer 8

says electrons must fill up orbitals, subshells, and shells in order of increasing energy.

Question 9

electromagnetic radiation

Answer 9

When electrons absorb , a form of energy, the electrons can jump to higher energy levels.

Question 10

Bohr model

Answer 10

The serves the purpose of understanding atomic structure rather than structural accuracy.

Question 11

Avogadros Number

Answer 11

is the number of atoms in a single mole of any given element.

Question 12

electrostatic force

Answer 12

The is the attraction between opposite charges and the strength can vary depending on now for the charges are from each other.

Question 13

subshell

Answer 13

A(n) is the shape of the space an electron can be found in.

Question 14

ionization energy

Answer 14

Once a shell is empty, the greatly increases because it is closer to the nucleus.

Question 15

mass spectrometry

Answer 15

determines the average mass for different isotopes of a specific element

Question 16

Coulomb’s Law

Answer 16

the closer an electron is to the nucleus, the stronger the attraction and the less potential energy there is.

Question 17

Pauli Exclusion Principle

Answer 17

states that when two electrons fill up an orbital, they must spin in opposite directions: clockwise and counterclockwise.

Question 18

Hund’s Rule

Answer 18

states that when electrons are filling the orbitals of the subshell, they will only have two in one orbital when it is not possible to have each electron in its own orbital.

Question 19

valence electrons

Answer 19

electrons in the outermost shell of an element

Question 20

cation

Answer 20

an ion that is positively charged after giving up an electron