OAT periodic Properties

What does the periodic law state

the chemical properties of the elements are dependent upon their atomic numbers

What are periods

rows

What are groups

columns

The electrons in the outer most shell are called

valance electrons

What are representative elements

elements that have either s or p orbitals as their outermost shell

What are nonrepresentative elements

elements that have a d orbital as their outer most shell or f

If an elements outer mot electron configuration is s²p⁴, how many valance electrons are there

2+4=6

What do all elements seek

to gain or loose electrons to achieve a stable, fully-filled electron configuration, like that of noble gases

In terms of protons, what happens as you go left to right on the periodic table

add 1 proton for each element

As you add protons, what happens to the electrons

they feel increasing nuclear attraction and become more tightly wound to the nucleus

The net positive charge from the nucleus as felt by the electrons is called

the effective nuclear charge

Going from top to bottom, electrons become

less tightly wound to the nucleus because the number of filled principal energy levels increases

Atomic radius decreases as you move

left to right and bottom to top across the periodic table.

Where will the atomic radius be largest

in the lower left corner of the periodic table

A change in the size of the electron cloud will change

the atomic radius and ionization energy

Altering the size of the nucleus does what in terms of atomic radius

nothing

Since the number of protons and electrons increase from left to right, the Z_eff(effective nuclear charge)

increases

The greater the positive charge the

greater the Z_eff, the closer the electrons are to the nucleus, and the smaller the atomic radius

From top to bottom Z_eff

decreases, atomic radius increases

What is ionization energy

the energy required to completely remove an electron from a gaseous atom or ion

Removing an electron always requires and is _

energy input, endothermic

What is the first ionization energy

the energy required to remove the first electron

What is the second ionization energy, is it typically more or less than the first

the energy needed to remove a second electron, typically greater than the first due to increased effective nuclear charge

When is the second ionization energy less than the first

if the removal of a second electron results in a fully filled or half filled valance shell

Ionization energy increases from

left to right, bottom to top(up)

Group IA have

low ionization energy because they would become noble gas configurations

What is electron affinity

the energy change that occurs when an electron is added to a gaseous atom and represents the ease with which the atom can accept an electron

The higher the Z_eff, the _ the electron affinity

greater

The common sign convention

a positive electron affinity value represents energy release when an electron is added

2nd or least common sign convention

a negative electron affinity represents a release of energy

Alkaline earth metals have _ electron affinity

low because their s orbital is filled

Halogens have _ electron affinities

high because adding an electron result in noble gas configuration (octet)

Achieving a stable octet involves

a release of energy

the strong attraction of the nucleus for electrons leads to

a high change in energy

What is electronegativity

the measure of attraction an atom has for electrons in a chemical bond

The greater an atoms electronegativity

the greater the attraction for bonding electrons

What is the most common electronegativity scale

Pauling electronegativity scale

0.7 most positive

0.4 most electronegative (F)

Electronegativity increases

from left to right and up the periodic table

What are the 3 classifications of elements

metal, nonmetal, metalloids or semimetals

Metals are known for their

malleability and ductility

Characteristics of metals

large atomic radius, low ionization energy, low electronegativity, and good energy conductors

Characteristics of nonmetals

small atomic radius, high ionization energy, high electronegativity, and are not good energy conductors

Metalloids include

boron, silicon, geranium, arsenic, antimony, and tellurium

Characteristics of metalloids

density, boiling points, and melting point fluctuate no real trends

electronegativity and ionization energy are found between metals and nonmetals

Reactivity of metalloids depend upon

the element they are reacting with

metal with nonmetal, nonmetal with metal

What reactions occur with ionic solutions

acid-base and oxidation-reduction

Cations are

positive

Anions are

negative

For elements that can form more than one cation, how is the charge indicated

with roman numerals after the element name

Cu⁺ is copper(I), and Cu²⁺is copper (II).

What can be added to indicate a lesser or greater positive charge respectively

-ous or -ic

For a monatomic anion how to you name it

drop the ending of the element name and add -ide

When do you add hypo-

when 1 oxygen is present in an oxyanion

When do you add per-

when 4 oxygens are present in an oxyanion

How do you name a lesser and greater oxyanion respectively

-ite for less oxygen, -ate for more oxygen

For polyatomic anions, how do you name compounds with 1 H

either hydrogen or bi-

How do you name polyatomic compounds with 2 hydrogens

dihydrogen

Metals typically form

positive ions

Nonmetals typically form

negative ions

2 exceptions of metals forming anion

permangantate and chromate

Alkali metals typically form

cations with 1+

Alkaline earth metals typically form

cations with 2+

Halogens typically form

anions with 1-

Hydrogen is its own group because

it can form H⁺ or a hydride ion

Alkali metals have

one loosely bound electron, low ionization energy and electronegativity

high reactivity with halogens expecially

Alkaline earth metals have

2 valance electrons, smaller atomic radii than alkali, low electronegativity and positive electron affinity

The electrons of alkaline earth metals can be removed to form

divalent cations

Carbon Group have

2 electrons in the p orbital, tend to not form ions but participate in electron sharing

Pnictogens or nitrogen group

form covalent bonds, commonly have a + charge and make nitrogen-containing compounds good bases

Chalcogens or oxygen group

require 2 electrons to complete octet, fairly electronegative and can also particpate in covalent bonding

Halogens

highly reactive nonmetals, need 1 electron, high electronegativity reactive with alkali metals to form crystals

Nobel gasses

nonreactive, complete octet, high ionization energy, no electronegativity

Transition metals have

high melting and boiling points, low electronegativities which allow oxidation states

Dissolved transition state metal ions can form_ with either or _

complex ions, water for hydration complex or nonmetals forming color

What causes d orbitals to split into 2 energy sublevels

the formation of complexes by transition metals

By splitting, the d orbitals allow

complexes to absorb certain frequencies of light

What are the frequencies not absorbed by the complexes

subtraction frequencies that give the complex the color