Chemistry: Chapter 6

Front 1

Principle Energy Level

Back 1

The major energy levels of an atom

Front 2

Principal Quantum Number (n)

Back 2

Assigned by the quantum mechanical model to indicate the relative sizes and energies of atomic orbitals.

n specifies the atom's major energy levels

as N increases, the orbital becomes larger, the electron spends more time farther from the nucleus and the atom's energy increases.

Front 3

Energy Sublevels (s, p, d, or f)

Back 3

The energy levels contained within a principal energy level.
s orbitals are spherical

p orbitals are dumbell-shaped.

not all d or f orbitals have the same shape.

Each orbital can contain, at most, two electrons.

Front 4

What are the four sections, or blocks, of the periodic table

Back 4

s-block
p-block
d-block
f-block

Front 5

What does each block represent?

Back 5

A sub-energy level

Front 6

What do elements in the s-block have in common?

Back 6

Filled or partially filled s orbitals

Front 7

What is the valence electron configuration of each element in group 1?

Back 7

Group 1 elements have partially filled s orbitals containing one valence electron and electron configurations ending in s(1)

Front 8

What is the valence electron configuration of each element in group 2?

Back 8

Group 2 elements have completely filled s orbitals containing two valence electrons and electron configurations ending in s(2)

Front 9

Why does the s-block span two groups of elements?

Back 9

Because s orbitals hold two electrons at most.

Front 10

Why does the p-block span six groups of elements?

Back 10

Because the three p orbitals can hold a maximum of six electrons.

Front 11

Why are there no p-block elements in period 1?

Back 11

because the p sublevel does not exist for the first principal energy level.

Front 12

What is the ending of the electron configuration of each element in group 4?

Back 12

??

Front 13

In what period does the first d-energy sublevel appear?

Back 13

??

Front 14

Why does the d-block span ten groups of elements?

Back 14

??

Front 15

What is the ending of the electron configuration of each element in group 3?

Back 15

??

Front 16

In what period does the first f-energy sublevel appear?

Back 16

??

Front 17

List the contributions made by Dmitri Mendeleev to the classification of elements and the development of the periodic table.

Back 17

1. Demonstrated a connection between atomic mass and elemental properties.
2. He predicted the existence an properties of undiscovered elements that were later found.
3. He left blank spaces in the table where he thought the undiscovered elements should go.

Front 18

List the contributions made by Henry Moseley to the classification of elements and the development of the periodic table.

Back 18

1. He discovered that atoms of each element contain a unique number of protons in their nuclei - the number of protons being equal to the atom's atomic number.
2. He arranged the elements in order of increasing atomic number.

Front 19

Periods

Back 19

A horizontal row of elements in the modern periodic table.

There are 7 periods.

Front 20

Periodic Law

Back 20

States that when the elements are arranged by increasing atomic number, there is a periodic repetition of their properties.

Front 21

Groups

Back 21

A vertical column of elements in the periodic table arranged in order of increasing atomic number.

Also called a family.

There are 18 groups,

Front 22

Representative Elements

Back 22

Elements from groups 1,2, and 13-18 in the modern periodic table, possessing a wide range of chemical and physical properties.

Front 23

Transition Elements

Back 23

Elements in groups 3-12 of the modern periodic table and are further divided into transition metals and inner transition metals.

Front 24

Metals

Back 24

Elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors on heat and electricity.

Front 25

Alkali Metals

Back 25

Group 1 elements, except for hydrogen, they are reactive and usually exist as compounds with other elements.

Front 26

Alkaline Earth Metals

Back 26

Group 2 elements in the modern periodic table and are highly reactive.

Front 27

Transition Metals

Back 27

An element in groups 3-12 that is contained in the d-block of the periodic table and, with some exceptions, is characterized by a filled outermost s orbital energy level n, and filled or partially filled d orbitals of energy level n -1.

Front 28

Inner Transition Metal

Back 28

Type of group B element that is contained in the f-block of the periodic table and is characterized by a filled outermost orbital, and filled or partially filled 4f and 5f orbitals.

Front 29

Lanthanide Series

Back 29

In the periodic table, the f-block elements from period 6 that follow the element lanthanum.

Front 30

Actinide Series

Back 30

In the periodic table, the f-block elements from period 7 that follow the element actinium.

Front 31

Nonmetals

Back 31

Elements that are generally gases or dull, brittle solids that are poor conductors of heat and electricity.

Front 32

Halogens

Back 32

A highly reactive group 17 element

Front 33

Noble Gases

Back 33

An extremely unreactive group 18 element

Front 34

Metalloids

Back 34

An element that has physical and chemical` properties of both metals and nonmetals.

Front 35

Atomic Size

Back 35

??

Front 36

Ionization Energy

Back 36

The energy required to remove an electron from a gaseous atom.

Generally increases in moving from left-to-right across a period and decreases in moving down a group.

Front 37

Electronegativity

Back 37

Indicates the relative ability of an element's atoms to attract electrons in a chemical bond.

Front 38

What are the 3 factors that influence ALL TRENDS?

Back 38

1.

Front 39

Atomic Size (Radius)

Back 39

how closely an atom lies to a neighboring atom.