Honors Chemistry: Unit 3

Fluorine (F)

Element with the largest electronegativity.

Hydrogen (H)

Element with the largest ionization energy.

Cesium (Cs)

Element with the largest atomic radius.

Anions

Negatively charged ions that are larger than the atoms from which they formed.

Atomic radii location

Elements with the largest atomic radii are found in the lower left-hand corner of the periodic table.

Ionization energy trend

Ionization energy tends to decrease as you move down a group on the periodic table.

Smallest atomic radii location

Elements with the smallest atomic radii are found in the upper right-hand corner of the periodic table.

Least electronegative elements

Alkali metals are generally the least electronegative elements.

Group with highest first ionization energy

Group 18 elements have the highest first ionization energy.

Electronegativity

Measure of the attraction an atom has for electrons in chemical bonds.

Period/Series

A horizontal row of elements on the periodic table.

Ionization energy definition

Energy required to remove an electron from an atom.

Most active metals location

Most active metals are located in the lower left corner of the periodic table.

Atomic radius trend down a group

Atomic radius tends to increase as one moves down a group.

Atomic radius trend across a period

Atomic radius tends to decrease as one moves left to right across a period.

Electronegativity trend down a group

Electronegativity tends to decrease as one moves down a group.

Ionization energy trend across a period

Ionization energy tends to increase as one moves left to right across a period.

Family/Group

A vertical column of elements on the periodic table.

Electronegativity trend across a period

Electronegativity tends to increase as one moves left to right across a period.

Smallest atomic radius among elements

Fluorine (F) is the smallest radius among the given elements.

Smallest ionization energy among elements

Lithium (Li) has the smallest ionization energy among the given elements.

Cations

Positively charged ions that are smaller than the atoms from which they formed.

Largest radius among elements

Lithium (Li) has the largest radius among the given elements.

Smallest radius among elements

Neon (Ne) has the smallest radius among the given elements.

Half-filled p sublevels

Found in the nitrogen group.

Ionization energy definition

Energy needed to remove the outermost electron from an atom.

Highest ionization energy among elements

Radon has the highest ionization energy among the given elements.

Atomic radius statement

The radius decreases as you move from left to right on the table.

Valence electrons in elements

Alkaline earth metals all have two valence electrons.

Atomic radius decrease reason

There are more protons pulling the electrons tighter as you move across a period.

Atom size increase when forming ion

Fluorine increases in size when forming its most common ion.

Highest electronegativity among elements

Sulfur has the highest electronegativity among the given elements.

Most reactive family

Halogens are the most reactive family of elements.

Lowest ionization energy among elements

Silver has the lowest ionization energy among the given elements.

Family that forms +2 charge ions

Alkaline earth metals form ions with a +2 charge.

Typical charge of aluminum

Aluminum typically forms a +3 charge.

Most reactive element among options

Lithium is the most reactive among the given elements.

Element with 7 valence electrons

Bromine has 7 valence electrons.

Largest radius among elements

Calcium has the largest radius among the given elements.

Atomic size decrease reason

More protons in the nucleus pull the energy level tighter, making atoms smaller.

Definition of ionization energy

Energy needed to remove the outermost electron from an atom.

Characteristics of a wave

Crest- peak of each wave; Trough- bottom of each wave; Wavelength- distance between two consecutive crests; Frequency- number of waves per second; Amplitude- distance from rest position to crest.

Quantum of energy

Small piece or bundle of energy that cannot be easily noticed.

Unique line spectrum reason

Each electron transition releases a specific wavelength of light, creating a unique line on the spectrum.

Wave-mechanical model of the atom

Electrons are located in orbitals where they are most likely found, around a small, dense, positively charged nucleus.

Photoelectric effect

High-energy wavelengths of light can free electrons from a metal.

Charge for main group elements

Alkali metals +1, Alkaline earth metals +2, Boron +3, Carbon +/- 4, Nitrogen -3, Oxygen -2, Halogens -1, Noble gases 0.

Reactivity of noble gases

Noble gases are not reactive because they already have a full valence level.

Valence electron role in bonding

Atoms gain, lose, or share electrons to achieve a full valence energy level.