Chapter 2: The Periodic Table (10%)

number of electron shells

(aka principal energy level, denoted by the principal quantum number n)

Elements in the same period/horizontal row all have the same WHAT?

number of valence shell electrons

Elements in the same group/vertical column all have the same WHAT?

metals

Metals vs. Nonmetals vs. Metalloids

Shiny (lustrous)

Conduct electricity well

Malleable

Ductile

metals

Metals vs. Nonmetals vs. Metalloids

Found on the left side and middle of the periodic table

high, Lithium, low

Metals

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

malleability

Metals

The ability of metals to be hammered into shapes

ductility

Metals

The ability of metals to be pulled or drawn into wires

low

Metals

Do metals have a HIGH or LOW effective nuclear charge (Z_eff)?

low

Metals

Do metals have a HIGH or LOW electronegativity?

large

Metals

Do metals have a SMALL or LARGE atomic radius?

small

Metals

Do metals have a SMALL or LARGE ionic radius?

low

Metals

Do metals have a HIGH or LOW ionization energy?

low

Metals

Do metals have a HIGH or LOW electron affinity?

nonmetals

Metals vs. Nonmetals vs. Metalloids

Dull

Poor conductors of electricity

Brittle

nonmetals

Metals vs. Nonmetals vs. Metalloids

Found on the right side of the periodic table

high

Nonmetals

Do nonmetals have a HIGH or LOW ionization energies?

high

Nonmetals

Do nonmetals have a HIGH or LOW electron affinities?

high

Nonmetals

Do nonmetals have a HIGH or LOW electronegativities?

small

Nonmetals

Do nonmetals have a SMALL or LARGE atomic radii?

large

Nonmetals

Do nonmetals have a SMALL or LARGE ionic radii?

metals

Metals vs. Nonmetals

More likely to give up electrons during bonding

metalloids

Metals vs. Nonmetals vs. Metalloids

Possess characteristics of both metals and nonmetals

Shiny yet brittle

Semiconductors

metalloids

Metals vs. Nonmetals vs. Metalloids

Found in a stair-step pattern starting with boron (B)

effective nuclear charge (Z_eff)

The actual felt pull that the outermost electrons of an element “feel”

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, less, atomic radii, increases, reduces

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

This means they are held _____ tightly by the nucleus.

This is because of the ________ _______ → the distance between the nucleus and the valence electrons _________, therefore _________ the force of attraction.

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 (aka an ion)

The distance from its nucleus to the outermost electron shell

Typically determined within a crystal lattice

metals, cations, nonmetals, anions

Metals vs. Nonmetals

__________ lose electrons and become positive (aka they become _______) while __________ gain electrons and become negative (aka they become ________)

larger

Smaller vs. Larger

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

smaller

Smaller vs. Larger

For metals closer to the metalloid line, they have a ________ ionic radius than the other metals

metalloid

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

smaller

Smaller vs. Larger

The ionic radii of cations (aka metals) is generally ________ than the atomic radii of their corresponding neutral atom

larger

Smaller vs. Larger

The ionic radii of anions (aka nonmetals) is generally ________ than the atomic radii of their corresponding neutral atom

ionization energy

The amount of energy required to remove an electron from the valence shell of a gaseous species

Always requires an input of heat (is endothermic)

smaller, smaller

Smaller vs. Larger

The 1st ionization energy (IE) will always be _______ than the 2nd IE which will always be ________ than the 3rd 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 group

greater, high

Lesser vs. Greater

The STRONGER the electrostatic pull (the higher the Z_eff) between the nucleus and the valence shell electrons, the _________ the energy release will be when an atom gains the electron (aka the atom has a _____ electron affinity)

electronegativity

An atom's inherent ability to attract electrons towards its nucleus in a chemical bond

increases, decreases

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

more

Less vs. 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

Alkali Metals vs. Alkaline Earth Metals vs. Transition Metals vs. Chalcogens vs. Halogens vs. Noble Gases

Typically take on an oxidation state of +1

Prefer to lose an electron to achieve a noble gas-like configuration

Have only 1 loosely-bound electron in their valence shell

React readily with nonmetals, especially halogens

Group 1A/1

EX: Lithium (Li), Sodium (Na)

alkaline earth metals

Alkali Metals vs. Alkaline Earth Metals vs. Transition Metals vs. Chalcogens vs. Halogens vs. Noble Gases

Take on an oxidation state of +2

Can lose 2 electrons to achieve noble gas-like configuration

Have 2 valence electrons

Group 2A/2

EX: Magnesium (Mg), Calcium (Ca)

alkali metals, alkaline earth metals

Alkali Metals vs. Alkaline Earth Metals vs. Transition Metals vs. Chalcogens vs. Halogens vs. Noble Gases

The most reactive of all metals

Not naturally found in their elemental neutral state (2)

chalcogens

Alkali Metals vs. Alkaline Earth Metals vs. Transition Metals vs. Chalcogens vs. Halogens vs. Noble Gases

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 6A/16

EX: Oxygen (O), Sulfur (S)

halogens

Alkali Metals vs. Alkaline Earth Metals vs. Transition Metals vs. Chalcogens vs. Halogens vs. Noble Gases

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 neutral state but rather as ions

Group 7A/17

EX: Fluorine (F), Chlorine (Cl)

noble gases

Alkali Metals vs. Alkaline Earth Metals vs. Transition Metals vs. Chalcogens vs. Halogens vs. Noble Gases

Have a fully filled valence shell in their standard state & 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 8A/18

EX: Neon (Ne), Helium (He)

transition metals

Alkali Metals vs. Alkaline Earth Metals vs. Transition Metals vs. Chalcogens vs. Halogens vs. Noble Gases

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 3-12

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 trends opposite of ALL the others