BJU Physical Science (6th ed.) - Chapter 4

How many periods are on the periodic table?

7

family

A column of elements in the periodic table having similar valence electron arrangement, resulting in similar chemical properties; also know as a GROUP.

Electronegativity

A measure of an element's ability to attract and hold electrons when bonded to other atoms

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons

Subscript

A number written slightly below and to the right of a chemical symbol that shows how many atoms of an element are in a compound.

period

A row in the periodic table of the elements; also called a SERIES

Group 1

Alkali metals +1

Group 2

Alkaline Earth Metals (+2)

Inner tansition metals

An element from either of two rows usually placed below the periodic table; a member of either the lanthanide or actinide series.

alkali meatals

An element in Group 1 of the periodic table, having one valence electron that it can easily lose to form a 1+ cation, making it extremely reactive

Nobel Gases

An element in Group 18 the periodic table having eight valence electrons that fill the outer energy level. (helium is and exception with only two.) With a full outer energy level, it is inert (i.e. nonreactive).

alkaline earth metal

An element in Group 2 of the periodic table, having two valence electrons that it tends to lose easily to become a 2+ cation, making it very reactive

metal

An element that is typically dense, solid, ductile, malleable, highly conductive, and chemically reactive, especially in the presence of nonmetal elements.

Nonmetal

An element that typically has four or more valence electrons and that does not exhibit the general properties of metals

Metaloids

An element with characteristics between those of metals and nonmetals; also called SEMICONDUCTORS

Tansition Metals

Any elements in Groups 3-12 of the periodic table typically having 1 or 2 valence electrons which it easily loses resulting in cations with charges of 1+ or 2+

mixed groups

Any of Groups 13-16 in the periodic table; so named because they contain metals, nonmetals, and metalloids. These groups are often named for the first element in the family

Place in chronological order the following people who contributed to the development of the periodic table: Berzelius, Döbereiner, Mendeleev, Moseley, Newlands.

Berzelius, Döbereiner, Newlands, Mendeleev, Mosley

Does CN represent the element copernicium (112) or a compound of carbon and nitrogen? Explain.

CN must represent a carbon-nitrogen compound. If this symbol was representing copernicium, then the second letter (n) would be lowercase.

Noble gases

Chemically inert

Halogens

Contains nonmetals, 7 valence electrons in it's outermost energy level. Very reactive

Mendeleev

Created the first periodic table. Arranged elements by increasing atomic mass, left blank spaces for undiscovered elements, used rows and columns

Berzelius

Developed the modern symbols for the elements, Xx or X

Atomic radius

Distance from the center of the nuclei to the outer most energy level

valence electrons

Electrons on the outermost energy level of an atom, they are available to bond, go with the numbers at the top of the periodic table

Lavoisier

Elements combined in reactions (oxygen to create fire, combustion)

Metals

Elements that are good conductors of electric current and heat.

Nonmetals

Elements that are poor conductors of heat and electric current

Metalloids

Elements that have properties of both metals and nonmetals.

Octaves/octetes

Every 8 elements repeated their trends when arranged by atomic mass

Newlands

Expanded triads to octets,

Boyle and Lavoisier

First real chemists

cesium (group #)

Group 1

alkali metals

Group 1, 1 electron in outer level, very reactive

List the group number for each element. a. cadmium (1 point)

Group 12

carbon (group #)

Group 14

Group 17

Halogen Family, 7 valence electrons, highly reactive

What was Berzelius's contribution to the study of elements?

He created a system of chemical symbols that were based on the name of the element and the number of atoms. This became the basis for our modern system.

2 changes made to Mendeleev's original periodic table to produce the one that we use today.

He originally put the elements in columns according to atomic mass. This resulted in elements with similar characteristics being in rows. Mendeleev changed his table to list the elements in rows according to their atomic masses. Later the table was ordered by atomic number instead of atomic mass.

Name a key contribution that Robert Boyle made to the study of Chemistry.

He rejected the Greek concept of matter being mixtures of the five classical elements. He instead promoted the concept of matter consisting of indivisible particles of specific elements. He also promoted scientific inquiry and experimentation.

Periods

Horizontal rows on the periodic table

Why is the periodic table shaped the way it is

It's separated by how many energy levels are in each. The groups are arranged by elements with similar electron arrangements

Why did Berzelius establish his system of chemical symbols?

Many chemists had created symbols to represent elements and compounds. Berzelius created his system of chemical symbols to standardize the symbols to make sharing information easier.

mixed groups

Metals, nonmetals, metalloids

Group 13-16

Mixed groups to find the number of valence electrons face elements take the group number and subtract 10

What told Mendeleev where he should leave spaces for missing numbers and traits on the periodic table

Periodic law

Original Periodic Law

Properties of elements are a periodic function of their atomic mass

alkaline earth metals

Slightly less reactive then alkali metals

atomic radius

The distance from the center of an atom's nucleus to its outermost energy level.

Using the periodic table, list two pairs of elements that would have been out of order on Mendeleev's periodic table (according to atomic mass) compared with our current table. Assume that scientists knew about all elements up to and including lead.

The pairs cobalt and nickel, argon and potassium, and tellurium and iodine would all have been out of order. (Accept any of these pairs.)

Define periodicity.

The repeated pattern of properties exhibited by elements when put in order of atomic mass or atomic number.

Where do the names of elements come from?

Their Greek and Latin roots, Greek/Roman gods (Thorium), people (Einsteinium), and places (Californium)

Of what elements did the ancient Greeks believe all matter consisted?

They believed that all matter formed from variable mixtures of earth, water, fire, air (or wind), and aether.

Why do we need a periodic table?

While the specific form of a table may not be required, scientists recognized the need for a system to organize the information about chemical elements. Without some form of organization, the volume of information would be overwhelming.

electron-dot notation

a representation of an element's ability to attract and hold electrons when bonded to other atoms

periodic table

a table of the elements used to display there properties

Family/Group

a vertical column of elements in the periodic table

valence electrons

an electron in the outermost energy level of a neutral atom

valence electron

an electron in the outermost energy level of an atom.

electron-dot notation

an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element's symbol

Halogen

an element in Group 17 of the periodic table having seven valence electrons. It easily gains an electron, forming a 1- anion, which causes it to be highly reactive.

inner transition metals

elements that appear below the main body of the periodic table

transition metals

elements that form a bridge between elements on the left and right sides of the periodic table

Group 18

noble gases

Alchemist

one who practices medieval chemistry or tries to change metals into gold, wack

periodic law

the law that states the properties of the elements vary with their atomic numbers in a regular, repeated pattern.

Modern Periodic Law

the properties of the elements are periodic functions of their atomic numbers

State the periodic law.

the properties of the elements change in a repeating way with their atomic numbers.

Group 3-12

transition metals, 1 or 2 valence electrons

Döbereiner

triads based on similar chemical properties, atomic mass, & density, he used atomic mass, so his science was faulty since they didn't know about isotopes