Chapter 2: The Periodic Table (10%)

principal energy level (n)

Rows are called periods and are based on the same ?

number of valence shell electrons

Columns are called groups and are based on the same ?

metals

elements that are shiny (lustrous), conduct electricity well, and are malleable and ductile

metals

types of elements found on the left side and middle of the periodic table

high, Lithium

metals generally have _____ boiling points and densities, but there are exceptions such as _________ which has a density about half of that of water.

malleability

the ability of metals to be hammered into shapes

ductility

the ability of metals to be pulled or drawn into wires

low

Do metals have a high or low effective nuclear charge?

low

Do metals have a high or low electronegativity?

large

Do metals have a small or large atomic radius?

small

Do metals have a small or large ionic radius?

low

Do metals have a high or low ionization energy?

low

Do metals have a high or low electron affinity?

nonmetals

elements that are dull, poor conductors of electricity, and are brittle

nonmetals

types of elements found on the right side of the periodic table

high

Do nonmetals have a high or low ionization energies?

high

Do nonmetals have a high or low electron affinities?

high

Do nonmetals have a high or low electronegativities?

small

Do nonmetals have a small or large atomic radii?

large

Do nonmetals have a small or large ionic radii?

metals

Which are more likely to give up electrons during bonding: metals or nonmetals?

metalloids

elements that possess characteristics of both metals and nonmetals

metalloids

types of elements that are found in a stair-step pattern starting with boron (B)

effective nuclear charge (Zeff)

the net positive charge experienced by electrons in the valence shell; the electrostatic attraction between the valence shell electrons and the nucleus; forms the foundation for all periodic trends

increases

Effective nuclear charge (Zeff) __________ from left to right across a period, with little change in value from top to bottom in a group

separated, increases

Valence electrons become increasingly ___________ from the nucleus as the principal energy level (n) __________ from top to bottom in a group

less

As the principal quantum number (n) increases down a group, the outermost electrons are held ______ tightly

atomic radius

Think of an atom as a cloud of electrons surrounding a dense core of protons and neutrons. The ________ ________ of an element is thus equal to ½ of the distance between the centers of two atoms of an element that are briefly in contact with each other.

decreases, increases

Atomic radius __________ from left to right across a period and __________ from top to bottom in a group

ionic radius

the size of a charged species

metals, nonmetals

When understanding ionic radii, know these generalizations: __________ lose electrons and become positive while ______________ gain electrons and become negative

larger

For nonmetals close to the metalloid line, they have a _________ ionic radius than their counterparts closer to Group VIIIA

smaller

For metals closer to the metalloid line, they have a __________ ionic radius than their counterparts of other metals

metalloid

the largest nonmetallic ionic radii and the smallest metallic ionic radii exist at the ___________ boundary

smaller

cations generally have a ________ ionic radii than their corresponding neutral atom

larger

anions generally have a ________ ionic radii than their corresponding neutral atom

ionization energy

the amount of energy necessary to remove an electron from the valence shell of a gaseous species; always requires an input of heat (is endothermic)

smaller, smaller

The first ionization energy (IE) will always be _______ than the second IE which will always be ________ than the third IE and so on

increases, decreases

ionization energy ____________ from left to right across a period and ___________ from top to bottom in a group

electron affinity

the amount of energy released when a gaseous species gains an electron in its valence shell; exothermic process that expels energy as heat

increases, decreases

electron affinity ____________ from left to right across a period and ___________ from top to bottom in a period

greater

the stronger the electrostatic pull (the higher the Zeff) between the nucleus and the valence shell electrons, the _________ the energy release will be when an atom gains the electron

electronegativity

a measure of the attractive force of the nucleus for electrons within a bond

increases, decreases

electronegativity ___________ from left to right across a period and ___________ from top to bottom in a group

more

The greater the electronegativity of an atom, the ______ it attracts electrons within a bond

lower

The lower the ionization energy, the _________ the electronegativity

alkali metals

Name the element group

typically take on an oxidation state of +1; prefer to lose an electron to achieve a noble gas-like configuration; have only one loosely bound electron in their valence shell; react readily with nonmetals, especially halogens; Group IA; examples include Lithium and Sodium

alkaline earth metals

Name the element group

take on an oxidation state of +2; can lose two electrons to achieve noble gas-like configuration; have two valence electrons; Group IIA, examples include Magnesium and Calcium

alklali metals, alkaline earth metals

Name the element group

the most reactive of all metals and therefore not naturally found in their elemental neutral state (2)

chalcogens

Name the element group

take on oxidation states of -2 or +6 (depending on whether they are nonmetals or metals, respectively) in order to achieve noble gas configuration; each have 6 valence electrons; extremely important for normal biological function; Group VIA; examples include Oxygen and Sulfur

halogens

Name the element group

typically take on an oxidation state of -1; prefer to gain an electron to achieve noble gas-like configuration; have the highest electronegativities; highly reactive especially towards alkali and alkaline earth metals; not naturally found in their elemental state but rather as ions; Group VIIA; examples include Fluorine and Chlorine

noble gases

Name the element group

have a fully filled valence shell in their standard state and prefer not to give up or take on additional electrons; have very high ionization energies and virtually nonexistent electronegativities and electron affinities; have extremely low boiling points and exist as gases at room temperature; Group VIIA; examples include Neon and Helium

transition metals

Name the element group

take on multiple oxidation states, which explains their ability to form colorful complexes with nonmetals in solution and their utility in certain biological systems; Groups 3 to 12

absorbed, subtraction frequencies, complementary color

When we perceive an object as a particular color, it is because the color is NOT __________. If an object absorbs a given color of light and reflects all others, our brain mixes these _____________ _______________ and we perceive the ________________ _________ of the frequency that was absorbed.

atomic radius

the period trend that acts opposite of all the others