Unit III

Question 1

Is a representation of what an atom could look based on the observations and scientific evidence that describes how atoms behave.

Answer 1

Atomic Model

Question 2

Considered the smallest particle of matter.

Answer 2

Atom

Question 3

Who wrote A New System of Chemical Philosophy?

Answer 3

John Dalton

Question 4

It is a particle smaller than an atom.

Answer 4

Subatomic Particle

Question 5

Who discovered Electrons?

Answer 5

J.J. Thomson

Question 6

Negatively charged particles.

Answer 6

Electrons

Question 7

What model did Thomson do?

Answer 7

Plum Pudding Model

Question 8

Who discovered protons?

Answer 8

Ernest Rutherfordium

Question 9

Atoms consists of a dense core called the _______.

Answer 9

Nucleus

Question 10

Positively charged particle inside the nucleus known as _________.

Answer 10

Proton

Question 11

Who made the planetary model?

Answer 11

Niels Bohr

Question 12

Who discovered the neutron?

Answer 12

James Chadwick

Question 13

It is equivalent to the number of protons in its nucleus.

Answer 13

Atomic Number (Z)

Question 14

The combined number of protons and neutrons present in its nucleus.

Answer 14

Mass Number

Question 15

Electrically charged atoms.

Answer 15

Ions

Question 16

When an atom gains an electron.

Answer 16

Anion

Question 17

When an atom loses an electron.

Answer 17

Cation

Question 18

The time it takes for half of a given sample of a particular isotope to decay on average is called its ___________.

Answer 18

half-life

Question 19

Describes the location and energy of the electrons in an atom.

Answer 19

Electron Configuration

Question 20

Used when describing the energy levels of electrons in atoms.

Answer 20

Quantum Number

Question 21

Specifies the energy of an electron and the size of the orbital.

Answer 21

Principal Quantum Number (n)

Question 22

Represents the shape of the sublevel.

Answer 22

Angular Momentum Quantum Number (l)

Question 23

Describes the orientation in space an orbital.

Answer 23

Magnetic Quantum Number

Question 24

Describes the spin of an electron.

Answer 24

Spin Quantum Number

Question 25

Pictorial representations of the electrons in an atom.

Answer 25

Orbital Diagrams

Question 26

It states that a lower energy should be filled first before the next higher energy orbital.

Answer 26

Aufbau Principle

Question 27

States that no two electrons can have exactly the same set of quantum numbers.

Answer 27

Pauli Exclusion Principle

Question 28

States that every orbital of the same energy must be singly occupied with one electron before any orbital is doubly occupied.

Answer 28

Hund’s Rule

Question 29

How many known elemente are there in the periodic table?

Answer 29

118 elements

Question 30

Elements can be arranged using the atomic weights with similar properties, which may be observed at a regular interval every after the seventh element. This is known as _________.

Answer 30

Law of Octaves

Question 31

Who wrote the book Principles of Chemistry?

Answer 31

Dmitri Mendeleev

Question 32

States that similar properties would repeat periodically when elements are arranged in increasing atomic number.

Answer 32

Periodic Law

Question 33

What are the three types of elements?

Answer 33

Metals, Metalloids, Nonmetal

Question 34

The outermost electrons of atoms.

Answer 34

Valence Electrons

Question 35

The horizontal arrangement in the periodic table is known as ____________.

Answer 35

Period or Series

Question 36

Vertical arrangement in the periodic table.

Answer 36

Groups

Question 37

Shows a pattern of the properties of elements based on their location and group.

Answer 37

Periodic Trends

Question 38

Is one-half the distance between the nuclei of two atoms.

Answer 38

Atomic Radius

Question 39

Amount of energy required to remove an electron.

Answer 39

Ionization Energy

Question 40

Ability of an element to attract valence electrons.

Answer 40

Electronegativity

Question 41

Ability of an atom to accept an electron.

Answer 41

Electron Affinity