ATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE

ATOMS

AND THE

PERIODIC

TABLE

CHAPTER 3

PHYSICAL

SCIENCE

Chapter 3 Vocabulary Words

 Nucleus Atomic number

 Proton Mass number

 Neutron Isotopes

 Electron Atomic mass unit (amu)

 Energy level Average atomic mass

 Orbital Metals

 Valence electron Nonmetals

 Periodic law Semiconductors

 Period Alkali metals

 Group Alkaline-earth metals

 Ionization Transition metals

 Ion Halogens

 Cation Noble gases

A. Atomic Structure

1.

What are atoms?

a. Atoms are tiny units that determine properties

of all matter.

b. Democritus was the first to suggest that the

universe was made of atoms, but couldn’t provide evidence to prove it!

c. 1808 John Dalton proposed the atomic theory

1. John Dalton’s Atomic Theory a. Every element is

made of tiny, unique particles called atoms that cannot be

subdivided.

b. Atoms of the same

element are exactly alike.

c. Atoms of different

elements can join to form molecules.

2. What’s in an Atom?

protons, neutrons, and electrons

1. nucleus: the center of an

atom made up of protons and neutrons

2. Protons: a positively

charged subatomic particle in the nucleus of an atom

3. Neutron: a neutral

subatomic particle in the nucleus of an atom

4. Electron: a tiny negatively

charged subatomic particle moving around outside the nucleus of an atom

5. The number of protons and electrons an atom has is unique for each element.

b. Atoms have no overall charge

1. Atoms don’t have a charge because they have an equal number of protons and electrons whose charges exactly cancel.

3. Models of the Atom

a. Bohr’s model compares electrons to planets

1. 1913 Niels Bohr suggested that electrons in an atom

move in set paths around the nucleus like the planets around the sun.

2. Energy level: any of the possible energies an electron

may have in an atom

3. Electrons must gain or lose energy to move up or

b. According to modern theory, electrons

behave more like waves

1. Since Bohr’s model couldn’t explain

everything, the modern model believes

electrons behave like waves on a vibrating string.

2. Don’t exactly know where the electrons are at,

but can calculate an area they are found

3. Electrons are found in orbitals within energy levels a. Orbitals: a region in an atom where there is a high probability of finding electrons

b. There are four different kinds of orbitals

4. Every atom has one or more valence electrons

a. Valence electron: an electron in the outermost energy level of an atom

B. A Guided Tour of the Periodic

Table

1. Organization of the Periodic Table

a. The periodic table groups similar elements together b. The order is based on the number of protons an atom

of that element has in its nucleus

c. Periodic law: properties of elements tend to change in

a regular pattern when elements are arranged in order of increasing atomic number, or number of protons in their atoms.

4. Using the periodic table to determine electronic arrangement

a. Period: a horizontal row of elements in the periodic table

b. Just as the number of protons increase left to right, so does the number of electrons

5. Elements in the same group have similar properties

a. Group (family): a vertical column of elements in the periodic table

b. Valence electrons determine properties c. Atoms in the same group have the same

2. Some Atoms Form Ions

a. Atoms that do not have filled outermost energy

levels may undergo ionization.

b. Ionization: the process of adding electrons to

or removing electrons from an atom or group of atoms

c. Atoms do this to fill their outermost energy

levels

d. Ion: an atom or group of atoms that has lost

or gained one or more electrons and therefore has a net electric charge

e. Cation: an ion with a positive charge 1. Caused by losing electrons

f. Anion: an ion with a negative charge

3. How do the Structures of Atoms Differ?

A. Atomic number

equals the number of protons

1. Atomic number: the number of protons in the nucleus of an atom 2. Each element has a

different number of proton.

B. Mass number equals the total number of subatomic particles in the nucleus

1. Mass number: the total number of

protons and neutrons in the nucleus of an atom

C. Isotopes of an element have different number of neutrons

1. Isotopes: any atoms having the same number of protons but different numbers of neutrons

D. Some isotopes are more common than others

E. Calculating the number of neutrons in an atom

1. Subtract atomic number from the mass

F. The mass of an atom

equal to one-twelfth of the mass of a carbon-12 atom

b. Proton and neutron

have a mass of 1amu

c. Average atomic mass:

the weighted average of masses of all

naturally occurring

isotopes of an element

1. Often found on the periodic table

C.

Families of Elements

1. How are Elements Classified?

a. Elements are either metals or nonmetals

b. Metals: the elements that are good conductors of heat

and electricity

c. Nonmetals: the elements that are usually poor conductors

d. Semiconductors: the elements that are intermediate conductors of heat and electricity

2. Metals

a. Alkali Metals

1. Alkali metals: the

highly reactive metallic elements located in

Group 1 of the periodic table

b. Alkaline-earth metals

1. Alkaline-earth metals: the reactive metallic

elements located in Group 2 of the

c. Transition metals

1. Transition metals: the metallic elements located in groups 3-12 of the periodic table

d. Synthetic elements

3. Nonmetals

a. Found on the right

side of the periodic table, except for

hydrogen

b. Carbon is found in

three different forms and can also form many compounds

c. Nonmetals and their compounds are plentiful on Earth

d. Chlorine is a halogen

that protects you

from harmful bacteria

1. halogen: the highly reactive elements

located in Group 17 of the periodic table

d. The noble gas neon is inert

1. Noble gases: the

unreactive gaseous elements located in Group 18 of the

e. Semiconductors are intermediate conductors of heat and electricity

f. Silicon is the most