Review Chapter 12 and 13

1. Always Soluble = a. Ionic Bond 2. Never Soluble = c. Metallic Bond 3. Sometimes Soluable = b. Covalent Bond

1. Always Soluble 2. Never Soluble 3. Sometimes Soluable a. Ionic Bond b. Covalent Bond c. Metallic Bond

1. Bonds only metals = b. Metallic 2. Bonds nonmetals and metals = c. Ionic 3. Bonds only nonmetals = a. Covalent

1. Bonds only metals 2. Bonds nonmetals and metals 3. Bonds only nonmetals a. Covalent b. Metallic c. Ionic

1. Brittle solids = c. Ionic 2. Typically liquids or gases = d. Molecular Covalent 3. Extremely hard solids = a. Network Covalent 4. Bendable and hard solids = b. Metallic

1. Brittle solids 2. Typically liquids or gases 3. Extremely hard solids 4. Bendable and hard solids a. Network covalent b. Metallic c. Ionic d. Molecular Covalent

1. Conducts electricity when dissolved = a Ionic 2. Never conducts electricity = b. covalent 3. Always conducts electricity = c. Metallic

1. Conducts electricity when dissolved 2. Never conducts electricity 3. Always conducts electricity a. Ionic b. Covalent c. Metallic

1. NaCl = a. Ionic 2. CO2 = c. Covalent 3. Fe = b. Metallic 4. Ge3N4 = d. Unable to tell

1. NaCl 2. CO2 3. Fe 4. Ge3N4 a. Ionic b. Metallic c. Covalent d. Unable to tell

1. The number of valance electrons = d. look at what group the element is in, the number corresponds to this. 2. The number of protons in an atom = b. Look at the atomic number of the element. 3. The number of neutrons in an atom = a. Take the atomic number of the element and subtract it from the mass number. 4. The oxidation number = e. There is a pattern on the periodic table. 5. The number of energy rings in an atom = c. These increase by one as you go down a group.

1. The number of valance electrons 2. The number of protons in an atoms 3. The number of neutrons in an atom 4. The oxidation number 5. The number of energy rings in an atom a. Take the atomic number of the element and subtract it from the mass number b. Look at the atomic number of the element. c. These increase by one as you go down a group. d. Look at what group the element is in, the number corresponds to this. e. There is a pattern on the periodic table.

56

A common isotope of iron has a mass number of 56. The total number of subatomic particles in the nucleus is: a. 26 b. 56 c. 30 d. 4

14

A neutrally charged atom of silicon has how many electrons? a. 7 b. 14 c. 28 d. Cannot be determined with the information given.

Lithium and fluorine atoms

An ionic bonds is most likely to form between: a. carbon and oxygen atoms. b. lithium and fluorine atoms. c. two oxygen atoms. d. nitrogen and oxygen atoms.

An ion.

At atom that acquires an electrical charge by gaining or losing electrons is known as: a. an ion b. a free radical. c. a hydrate d. a monatomic molecule

The same number of protons but a different number of neutrons.

Atoms of the same element may contain: a. The same number of neutrons but a different number of protons. b. The same number of protons but a different number of neutrons. c. A different number of protons and a different number of neutrons. d. The same number of electrons but a different number of protons.

True

Atoms that gain electrons are known as anions. True or False

False (gain)

Atoms that lose electrons are known as anions. True or False

Ions

Atoms that lose or gain electrons are called: a. alloys b. mixtures c. ions d. elements

Ionic

Chemical bonds formed by transferring electrons are known as _________ bonds.

Huge

Compared to electrons, the mass of proton is _____.

Much smaller mass and opposite charge.

Compared to protons, electrons have: a. Much smaller mass and opposite charge. b. About the same mass and opposite charge. c. Much larger mass and the same charge. d. Much larger mass and opposite charge.

When electrons are shared between two atoms.

Covalent bonding occurs: a. in salt like NaCl b. when electrons are shared between two atoms. c. only when electrons are shared between two identical atoms. d. when electrons are transferred from one atom to another.

A metalloid and oxygen

Covalent bonds would most likely form between: a. an alkali metal and helium b. magnesium and a halogen c. a metalloid and oxygen d. sodium and chlorine

An oxidation number of 1+

Elements in the first column of the periodic table are known as alkali metals. What do these elements have in common when ionized? a. An oxidation number of 1- b. An oxidation number of 1+ c. An oxidation number of 2- d. An oxidation number of 2+

8

How many neutrons does a carbon atoms with a mass number of 14 and an atomic number of 6, have?

3

How many valence electrons are in an atom of aluminum, atomic number 13? a. 1 b. 2 c. 3 d. 4

True

Metals tend to lose electrons. True or False

False (metals)

Nonmetals tend to gain electrons and become positive ions. True or False

Loses, gains

Sodium forms an ionic bond with chlorine when sodium ____ an electron and chlorine _____ an electron. a. shares, shares b. loses, gains c. gains, loses d. loses, loses

Loses two electrons.

The Mg atom becomes the ion, Mg2+, when it: a. gains two electrons b. loses two electrons c. gains two protons d. loses two protons

Lithium, atomic number 3

The atom of the element most likely to bond with a single atom of fluorine, atomic number 9 is: a. Lithium, atomic number 3. b. Beryllium, atomic number 4. c. Boron, atomic number 5. d. Carbon, atomic number 6.

The weighted average of the isotopes of that element.

The average atomic mass of an element is a. The number of protons plus the number of neutrons. b. The weighted average of the isotopes of that element. c. The weighted average of the ions of that element. d. The number of neutrons in that element.

Ca2+ and Cl-

The compound CaCl2 contains which of the following ions? a. Ca+ and C- b. Ca2+ and Cl2- c. Ca2+ and Cl- d. Ca4+ and Cl4+

Valence

The electron in the highest unfilled energy level of an atom are referred to as the _______ electrons.

Charge

The fundamental property of matter that can be either positive or negative is _______.

7

The most common oxidation number for an element in the second period is 3-. The atomic number of the element is: a. 3 b. 5 c. 7 d. 11

Have completely filled energy levels.

The nobel gases such as helium and xenon do not form chemical bonds with other elements because they: a. Have completely filled energy levels. b. Are chemically unstable. c. Are unusually large atoms. d. have been around longest on Earth.

1-

The oxidation number for chlorine (Cl) is ____.

Oxidation

The quantity indicating the charge on an atom when an electron is lost, gained or, shared during bond formation is called the _________ number.

Mass number

The total number of protons and neutrons in the nucleus of an atom are identified by a number called the _________.

Hydrogen and Oxygen.

Two elements are normally gases at room temperature. They are: a. Mercury and Bromine b. Hydrogen and Oxygen c. Water and Alcohol d. Boron and Magnesium

Al(OH)3

What is the chemical formula for a compound that contains the aluminum ion (Al3+) and the hydroxide ion (OH-)? a. Al(OH)3 b. AlO3H3 c. AlOH3 d. None of the above.

The number of protons

What, in an atom, is unique to each element? a. the number of electrons b. the number of protons c. the number of neutrons d. the mass number

Ionic BeS Beryllium sulfide

When we combine Beryllium (Group 2A) and Sulfur (Group 6A): _____ bonding is used _____ is the chemical formula _____ is the name of the compound

Ionic MgF2 Magnesium fluoride

When we combine Magnesium (Group 2A) and Fluorine (Group 7A): _____ bonding is used _____ is the chemical formula _____ is the name of the compound

Groups 1B-8B

Where are the transition elements located on the periodic table? a. Groups 1A-2A b. Groups 3A- 12A c. Groups 10A- 15A d. Groups 1B-8B

Valence electrons may be lost or gained by an atom when bonding occurs with another.

Which of the following is TRUE for valence electrons? a. Valence electrons are always located in the innermost energy level. b. Valence electrons may be lost or gained by an atom when bonding occurs with another.

The number of protons might be different between the two isotopes.

Which of the following statements about two isotopes of the same element is FALSE? a. The number of neutrons may be different between the two isotopes. b. One isotope might be radioactive while the other isotope might be stable. c. One isotope might have a larger mass than another isotope. d. The number of protons might be different between the two isotopes.

All Lithium atoms contain the same number of protons.

Which of the following statements is the most accurate? a. All lithium atoms contain the same number of protons. b. All lithium atoms contain the same number of neutrons. c. All lithium atoms have the same mass. d. The sum of protons plus neutrons is the same in all lithium atoms.

All of the above.

Which statement below correctly describes the relationship between electrons and their energy levels? a. An electron's energy must match one of the energy levels in an atom. b. Each energy level can hold only a certain number of electrons. c. Electrons added to an atom settle into unfilled positions nearest the nucleus. d. All of the above.

They have an oxidation number of 2+

Which statement is NOT TRUE about elements in group 6A? a. They need two electrons to complete their octet. b. They have an oxidation number of 2-. c. They have an oxidations number of 2+. d. They have six valence electrons.