Chemistry Ch.6 review

Binary ionic compounds

1. Consists of only two elements 2. Name the positive ion (the cation +) 3. Name the negative ion (the anion -), changing the ending to -ide 4. When metals that can form more than one type of ion are in a compound, use a Roman numeral in parentheses after the name of the metal to show the charge

Properties of ionic compounds

1. High melting and boiling points 2. Hard -not easily crushed 3. Conduct electricity when melted or dissolved because the ions are free to bond

Properties of covalent compounds

1. Lower melting and boiling points 2. Many covalent compounds are volatile liquids or gases 3. Softer - easier to crush 4. Are not conductors of electricity

Properties of metals

1. Luster 2. Conductors 3. Malleable 4. Ductile

Ternary ionic compounds

1. Made up of three or more elements 2. Name the cation then name the Polyatomic anion wing out changing the ending to "ide"

Molecular compounds

1. The elements are named in the order they appear in the formula 2. Prefixes are used to denote the number of atoms of each element in the molecule. An exception is that the first element named is given a prefix only if there is more than one atom of that element in the molecule 3. The "o" or "a" at the end of a prefix is dropped when the word following the prefix begins with a vowel 4. The last element's ending is changed to -ide

1.7

A bond's character is more than 50% ionic if the Electronegativity difference between the two atoms is greater than

A. Nuclei

A chemical bond between atoms results from the attraction between valence electrons and _____ of different atoms. A. Nuclei B. Inner electrons C. Isotopes D. Lewis structures

Ionic bond

A chemical bond that results from the electrostatic attraction between positive and ionic bond negative ions is called a(n)

B. A shared electron pair

A covalent bond consists of A. A shared electron B. A shared electron pair C. Two different ions D. An octet of electrons

B. Polar

A covalent bond in which there is an unequal attraction for the shared electron is A. Nonpolar B. Polar C. Ionic D. Dipolar

D. Absorb and re-emit the light

As light strikes the surface of a metal, the electrons in the electron sea A. Allow the light to pass through B. Become attached to particular positive ions C. Fall to lower energy levels D. Absorb and re-emit light

Anion

Atom gains electrons to become - charged

Cation

Atom loses electrons to become + charged

Electrons dot diagram

Atom's symbol surrounded by dots to represent its valence electrons

C. High Electronegativity

Atoms with a strong attraction for electrons they share with another atom exhibit A. Zero Electronegativity B. Low Electronegativity C. High Electronegativity D. Lewis Electronegativity

Polar covalent

Between 1.7 and 0.3

C. Polar covalent

Bonds that possess between 5% and 50% ionic character are considered to be A. Ionic B. Pure covalent C. polar covalent D. Non-polar covalent

Covalent

Compounds that have weaker forces holding molecules together

Polyatomic ions

Covalently bonded group of ions with a charge

Both nuclei attracted to pair of electrons being shared

Describe how a covalent bond holds two atoms together.

>EN more - the end will be & - <EN more + the end will be & +

Describe the electron distribution in a polar-covalent bond and its effect on the partial charges of the compound.

Electrostatic forces between cations and anions

Describe the force that holds two ions together in an ionic bond.

Lewis Structure

Diagram representing the arrangement of valence electrons Ina molecule

Metallic bond

Electrons are delocalized (creates "sea of electrons"

No polar covalent bonds

Electrons are shared equally because atoms have the same electronegativities

Polar covalent bonds

Electrons are shared unequally, creating partially charged ends or pols

Covalent bond

Electrons are shared, forming molecules

Sometimes 1 diagram doesn't accurately reflect what the molecule looks like. (The resonance structures show delocalized electrons)

Explain why resonance structures are used instead of Lewis structures to correctly model certain molecules.

Strong

Forces hold the ions together

Chemical bond

Forms when 2 or more atoms arrange valence elctrons to increase stability

Ionic bond

Forms when valence electrons are transferred from one atom to another. Electrostatic once which holds a cation and an anion together in an ionic compound

Ionic

Greater than or equal to 1.7

Above 1.7 - ionic because the electron is transferred not shared

How can electronegativity be used to distinguish between an ionic bond and a covalent bond?

They are free to move (delocalized)

How does the behavior of electrons in metals contribute to the metal's ability to conduct electricity and heat?

Ionic bond

If a bond's character is more than 50% ionic, then the bond is called a(n)

Polar covalent

If electrons involved in bonding spend most of the time closer to one atom rather than the other, the bond is

A. Nonpolar covalent

If two covalent oh bonded atoms are identical, the bond is identified as A. Nonpolar covalent B. Polar covalent C. Ionic D. Polar

D. Negative ions

In a crystal of an ionic compound, each cation is surrounded by a number of A. Molecules B. Positive ions C. Dipoles D. Negative ions

A. Increases

In general, the strength of the metallic bond ____ moving from left to right on any row of the periodic table. A. Increases B. Decreases C. Remains the same D. Varies

Crystal lattice

In ionic compounds the ions are arranged in a

B. Shared by all surrounding atoms.

In metals, the valence electrons are considered to be A. Attached to particular positive ions B. Shared by all surrounding atoms. C. Immobile D. Involved in covalent bonds

No polar covalent

Less than or equal to 0.3

D. All of the above

Mobile electrons in the metallic bond are responsible for A. Luster B. Thermal conductivity C. Electrical conductivity D. All of the above

Hydrogen and Boron

Name two elements that form compounds that can be exceptions to the octet rule.

Electronegativity

Property that tells how strong an atom's attraction is for electrons

Valence electrons

The electrons involved in the formation of a chemical bond are called

A. Chemical bonds

The fact that metals are malleable and ionic crystals are brittle is best explained in terms of their A. Chemical bonds B. London forces C. Enthalpies of vaporization D. Polarity

B. Weaker than the attractive forces among formula units in ionic bonding

The forces of attraction between molecules in a molecular compound are generally A. Stronger than the attractive forces among formula units in ionic bonding B. Weaker than the attractive forces among formula units in ionic bonding C. Approximately equal to the attractive forces among formula units in ionic bonding D. Equal to zero

A. Ionic character

The greater the Electronegativity difference between two atoms bonded together, the greater the bond's percentage of A. Ionic character B. Nonpolar character C. Metallic character D. Electron sharing

B. Lower in potential energy

The lattice energy of compound A is greater in magnitude than that of compound B. What can be concluded from this fact? A. Compound A is not an ionic compound B. It will be more difficult to break the bonds in compound A than those in compound B. C. Compound B has larger crystals than compound A. D. Compound A has larger crystals than compound B.

A. Formula unit

The notation for sodium chloride, NaCl, stands for one A. Formula unit B. Molecule C. Crystal D. Atom

Electronegativity difference

What property of the two atoms in a covalent bond determines whether or not the bond will be polar?

Lattice energy

What type of energy best represents the strength of an ionic bond?

Ionic (cation & ion) Covalent (nonmetals w/o the PA1)

What types of bonds are present in an ionic compound that contains a Polyatomic ion?

C. Do not break

When a metal is drawn into a wire, the metallic bonds A. Break easily B. Breaks with difficultly C. Do not break D. Become ionic bonds