Chemistry Unit 5: Ionic Bonds and Compounds

How are Ionic bonds formed?

When atoms of a metal transfer to a nonmetal

What are Ionic bonds?

The electrostatic force that holds oppositely charged particles together in an ionic compound

What is a formula unit?

The simplest ratio of ions (overall charge is 0)

What is a monatomic ion?

A one-atom ion

Mono- one

What does a subscript show?

The number of ions in a formula unit

What compounds have a neutral charge?

Ionic compounds

How can some compounds be neutral?

Electrons must be equal to the electrons gained

What are polyatomic ions?

Multiple atom ions

Poly- many

How do ions form into a crystalline lattice?

Positive and negative ions lineup and pack tight

What are electrolytes?

An ionic compound whose aqueous solution conducts an electric current

Why are Ionic compounds difficult to break apart?

Complex lattices with high melting and boiling points

What are the properties of ionic compounds?

Forms crystalline lattices, strong, high melting and boiling points, brittle, conducts electricity when dissolved in a liquid

What is an endothermic reaction?

Energy absorbed during a chemical reaction

What is an exothermic reaction?

Energy is released

What does the attraction of positive and negative ions form?

A more stable system than individuals

What happens when same energy is put into lattice?

They seperate

What is lattice energy?

Energy required to separate compound’s ions

An ion with a high charge has a ___ lattice energy

High

An ion with a low charge has ___ lattice energy

Low

Are pure metals iconically bonded?

NO but they have lattices when solid

What is the electron sea model?

The idea that all metal atoms in a metallic solid contributes their valence electrons to form a sea of electrons

What are delocalized electrons

Electrons in metallic bonding because they are free to move

What is metallic bonding?

Attraction of a metallic cation for delocalized electrons

What are the properties of metals?

High melting point, low boiling point, ductile, malleble, conductors

What is an alloy?

Mixture of elements with metallic properties

What is substitutional

Replacing one with another

What is interstitial?

Filling in gaps between larger atoms

What are the properties of metal alloys?

Harder, stronger, less ductile

What are valence electrons?

Electrons in the outermost orbitals

What parts of the periodic table are Representative elements?

S and P block

What sections of the periodic table are transition elements?

D block

What section of the periodic table are inner transition metals?

F block

What are group 1?

Alkali metals with 1 valence electron

What are group 2?

Alkaline earth metals with 2 valence electrons

What are groups 3-12?

Transition metals

What are lanthanide and actinide?

Inner transition metals

What are group 17?

Halogens with 7 valence electrons

What are group 18?

Noble gases with 8 valence electrons

What are the properties of metals?

Hard, shiny, solid, malleable, ductile, loses electrons, good heat conductors

What are the properties of non metals?

Upper right on pt, gases/brittle solids, poor heat conductors

What are the properties of metalloids?

Semimetals, staircase on pt, metal and nonmetal characteristics

What is electronegativity?

the ability to attract electrons to form a bond

What is the periodic table trend for electronegativity?

Increases up and to the right

What are the periodic table trends for ionization energy?

Increases up and to the right

What is ionization energy?

The amount of energy needed to remove an electron from a bond

What is atomic radi?

The distance between nucleus and outermost electron shell?

What are the periodic trends for atomic radi?

Increases down and to the left

How do you predict which element will have the highest ionization energy?

1. list electron configuration

2. whichever has the least amount of valence electrons have the highest ionization energy