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Chapter Introduction Lesson 1 Electrons and Energy Levels Lesson 2 Compounds, Chemical Formulas, and Covalent Bonds Lesson 3 Ionic and Metallic Bonds Chapter Wrap-Up
Chapter Menu
Chapter Introduction
Lesson 1 Electrons and Energy Levels
Lesson 2 Compounds, Chemical Formulas, and Covalent Bonds
Lesson 3 Ionic and Metallic Bonds
Chapter Wrap-Up
Chapter Introduction
How do elements join together to form chemical bonds?
Chapter Introduction
What do you think?
Before you begin, decide if you agree or disagree with each of these statements. As you view this presentation, see if you change your mind about any of the statements.
Chapter Introduction
1. Elements rarely exist in pure form. Instead, combinations of elements make up most of the matter around you.
2. Chemical bonds that form between atoms involve electrons.
Do you agree or disagree?
Chapter Introduction
3. The atoms in a water molecule are more chemically stable than they would be as individual atoms.
4. Many substances dissolve easily in water because opposite ends of a water molecule have opposite charges.
Do you agree or disagree?
Chapter Introduction
5. Losing valence electrons can make some atoms more chemically stable.
6. Metals are good electrical conductors because they tend to hold onto their valence electrons very tightly.
Do you agree or disagree?
Lesson 1 Reading Guide - KC
• How is an electron’s energy related to its distance from the nucleus?
• Why do atoms gain, lose, or share electrons?
Electrons and Energy Levels
Lesson 1 Reading Guide - Vocab
• chemical bond
• valence electron
• electron dot diagram
Electrons and Energy Levels
Lesson 1-1
• Elements on the periodic table are organized in periods (rows) and groups (columns).
• The periodic table lists elements in order of atomic number, which increases from left to right as you move across a period.
The Periodic Table
Lesson 1-1
The three main regions of elements on the periodic table classify elements as metals, nonmetals, or metalloids.
Lesson 1-1
The Periodic Table (cont.)
• Except for hydrogen, elements on the left side of the table are metals.
• Nonmetals are on the right side of the table.
• Metalloids form the narrow stair-step region between metals and nonmetals.
Lesson 1-2
• A chemical bond is a force that holds two or more atoms together in a compound.
• Atoms contain protons, neutrons, and electrons.
• Each proton has a positive charge; each neutron has no charge; and each electron has a negative charge.
Atoms Bond
Lesson 1-2
Protons and neutrons are in an atom’s nucleus. Electrons move around the nucleus.
Lesson 1-2
• The atomic number of an element is the number of protons in each atom of that element.
• An electron moves around the nucleus at a distance that corresponds to its amount of energy.
Atoms Bond (cont.)
Lesson 1-2
• Areas of space in which electrons move around the nucleus are called energy levels.
• Electrons closest to the nucleus have the least amount of energy. Electrons farthest from the nucleus have the greatest amount of energy.
Atoms Bond (cont.)
Lesson 1-2
Atoms Bond (cont.)
How is an electron’s energy related to its position in an atom?
Lesson 1-2
• The attraction between the positive nucleus of one atom and the negative electrons of another atom is what creates a chemical bond.
• A valence electron is an outermost electron of an atom that participates in chemical bonding.
Atoms Bond (cont.)
Lesson 1-2
The number of valence electrons in each atom of an element can help determine the type and number of bonds that an atom can form.
Atoms Bond (cont.)
valence
from Latin valentia, means “strength, capacity”
Lesson 1-2
The periodic table can tell you how many valence electrons an atom has.
Lesson 1-2
In 1916 an American chemist named Gilbert Lewis developed the electron dot diagram, a model that represents valence electrons in an atom as dots around the element’s chemical symbol.
Atoms Bond (cont.)
Lesson 1-2
• Atoms with eight valence electrons are chemically stable and do not easily react with other atoms.
• Atoms that have between one and seven valence electrons are reactive or chemically unstable and easily bond with other atoms to form chemically stable compounds.
Atoms Bond (cont.)
Lesson 1-2
• The elements in group 18 are called noble gases.
• With the exception of helium, noble gases have eight valence electrons and are chemically stable.
Atoms Bond (cont.)
Lesson 1-2
Atoms gain, lose, or share valence electrons and become chemically stable.
Lesson 1-2
Atoms Bond (cont.)
Why do atoms gain, lose, or share electrons?
Lesson 1 - VS
• Electrons are less strongly attracted to a nucleus the farther they are from it, similar to the way a magnet attracts a paper clip.
Lesson 1 - VS
• Electrons in atoms are in energy levels around the nucleus. Valence electrons are involved in chemical bonding.
Lesson 1 - VS
• All noble gases, except He, have four pairs of dots in their electron dot diagrams. Noble gases are chemically stable.
Lesson 1 – LR1
A. the left side
B. the right side
C. the middle
D. all of the above
Where on the periodic table are nonmetals located?
Lesson 1 – LR2
A. electron dot diagram
B. periodic table
C. neutron
D. energy levels
Which term refers to areas of space in which electrons move around the nucleus?
Lesson 1 – LR3
A. metalloids
B. valence electrons
C. noble gases
D. metals
All of the elements in group 18 are called what?
Lesson 1 - Now
1. Elements rarely exist in pure form.
Instead, combinations of elements
make up most of the matter around
you.
2. Chemical bonds that form between
atoms involve electrons.
Do you agree or disagree?
Lesson 2 Reading Guide - KC
• How do elements differ from the compounds they form?
• What are some common properties of a covalent compound?
• Why is water a polar compound?
Compounds, Chemical Formulas, and Covalent Bonds
Lesson 2 Reading Guide - Vocab
• covalent bond
• molecule
• polar molecule
• chemical formula
Compounds, Chemical Formulas, and Covalent Bonds
Lesson 2-1
• Compounds are chemical combinations of different types of atoms.
• Chemical bonds join atoms together.
From Elements to Compounds
Lesson 2-1
From Elements to Compounds (cont.)
bond
Science Use a force that holds atoms together in a compound
Common Use a close personal relationship between two people
Lesson 2-1
From Elements to Compounds (cont.)
How is a compound different from the elements that make it up?
Lesson 2-2
• A covalent bond is a chemical bond formed when two atoms share one or more pairs of valence electrons.
• A compound formed from many covalent bonds is called a covalent compound.
Covalent Bonds—Electron Sharing
Lesson 2-2
Atoms with less than eight valence electrons become chemically stable by forming a chemical bond.
Lesson 2-2
• A single covalent bond exists when two atoms share one pair of valence electrons.
• A double covalent bond exists when two atoms share two pairs of valence electrons
• A triple covalent bond exists when two atoms share three pairs of valence electrons.
Covalent Bonds—Electron Sharing (cont.)
Lesson 2-2
The more valence electrons that two atoms share, the stronger the covalent bond is between the atoms.
Lesson 2-3
• When two or more atoms share valence electrons, they form a stable covalent compound.
• Covalent compounds usually have low melting points and low boiling points.
• They are usually gases or liquids at room temperature, but they can also be solids.
• Covalent compounds are poor conductors of thermal energy and electricity.
Covalent Compounds
Lesson 2-3
Covalent Compounds (cont.)
What are some common properties of covalent compounds?
Lesson 2-3
• A molecule is a group of atoms held together by covalent bonding that acts as an independent unit.
• A molecule that has a partial positive end and a partial negative end because of unequal sharing of electrons is a polar molecule.
Covalent Compounds (cont.)
Lesson 2-3
Covalent Compounds (cont.)
polar
from Latin polus, means “pole”
Lesson 2-4
Atoms of a polar molecule share their valence electrons unequally.
Lesson 2-4
Atoms of a nonpolar molecule share their valence electrons equally.
Lesson 2-4
Covalent Compounds (cont.)
Why is water a polar compound?
Lesson 2-3
• A chemical formula is a group of chemical symbols and numbers that represent the elements and the number of atoms of each element that make up a compound.
• A chemical formula describes the types of atoms in a compound or a molecule, but it does not explain the shape or appearance of the molecule.
Covalent Compounds (cont.)
Lesson 2-4
Chemical formulas and molecular models provide information about molecules.
Lesson 2 - VS
• A chemical formula is one way to show the elements that make up a compound.
Lesson 2 - VS
• A covalent bond forms when atoms share valence electrons. The smallest particle of a covalent compound is a molecule.
Lesson 2 - VS
• Water is a polar molecule because the oxygen and hydrogen atoms unequally share electrons.
Lesson 2 – LR1
A. covalent bond
B. chemical formula
C. compound
D. polar molecule
Which term refers to chemical combinations of different types of atoms?
Lesson 2 – LR2
A. single covalent bond
B. double covalent bond
C. triple covalent bond
D. none of these
When two atoms share one pair of valence electrons, which of the following exists?
Lesson 2 – LR3
A. covalent bond
B. polar molecule
C. nonpolar molecule
D. covalent compound
Which term refers to a molecule that has a partial positive end and a partial negative end because of unequal sharing of electrons?
Lesson 2 - Now
3. The atoms in a water molecule are
more chemically stable than they would
be as individual atoms.
4. Many substances dissolve easily in
water because opposite ends of a
water molecule have opposite charges.
Do you agree or disagree?
Lesson 3 Reading Guide - KC
• What is an ionic compound?
• How do metallic bonds differ from covalent and ionic bonds?
Ionic and Metallic Bonds
Lesson 3 Reading Guide - Vocab
• ion
• ionic bond
• metallic bond
Ionic and Metallic Bonds
Lesson 3-1
An ion is an atom that is no longer electrically neutral because it has lost or gained valence electrons.
Understanding Ions
ion
from Greek ienai, means “to go”
Lesson 3-1
• Because electrons have a negative charge, losing or gaining an electron changes the overall charge of an atom.
• Atoms that lose valence electrons become ions with a positive charge.
• Metal atoms, such as sodium, become more stable when they lose valence electrons and form a chemical bond with a nonmetal.
Understanding Ions (cont.)
Lesson 3-1
Sodium atoms have a tendency to lose a valence electron. Chlorine atoms have a tendency to gain a valence electron.
Lesson 3-1
• Atoms are electrically neutral because they have the same number of protons and electrons.
• Once an atom gains or loses electrons, it becomes a charged ion.
Understanding Ions (cont.)
Lesson 3-2
• When forming a compound, the nonmetal atoms gain the electrons lost by the metal atoms.
• The attraction between positively and negatively charged ions in an ionic compound is an ionic bond.
Ionic Bonds—Electron Transferring
Lesson 3-2
An ionic bond forms between Na and Cl when an Na atom transfers an electron to a Cl atom.
Lesson 3-2
Ionic Bonds—Electron Transferring (cont.)
What holds ionic compounds together?
Lesson 3-3
• Individual ions in an ionic compound are strongly attracted to each other.
• Covalent compounds are made up of many molecules.
• When nonmetal ions bond to metal ions in an ionic compound there is a large collection of oppositely charged ions and no molecules.
Ionic Compounds
Lesson 3-4
• A metallic bond is a bond formed when many metal atoms share their pooled valence electrons.
• Valence electrons in metals are not bonded to one atom.
• Instead, a “sea of electrons” surrounds the positive ions.
Metallic Bonds—Electron Pooling
Lesson 3-4
Valence electrons are free to move among all the aluminum (Al) ions.
Lesson 3-4
Metallic Bonds—Electron Pooling (cont.)
How do metal atoms bond with one another?
Lesson 3-4
• Metals are good conductors of thermal energy and electricity.
• Metals are shiny because the valence electrons at the surface of a metal interact with light.
Metallic Bonds—Electron Pooling (cont.)
Lesson 3 - VS
• Metal atoms lose electrons and nonmetal atoms gain electrons and form stable compounds. An atom that has gained or lost an electron is an ion.
Lesson 3 - VS
• An ionic bond forms between positively and negatively charged ions.
Lesson 3 - VS
• A metallic bond forms when many metal atoms share their pooled valence electrons.
Lesson 3 – LR1
A. covalent compound
B. proton
C. ion
D. molecule
Which of these describes an atom that is no longer electrically neutral because it has lost or gained valence electrons ?
Lesson 3 – LR2
A. ionic bond
B. metallic bond
C. covalent compound
D. ionic compound
What is a bond formed when many metal atoms share their pooled valence electrons?
Lesson 3 – LR3
A. valence electrons
B. covalent compound
C. ionic compound
D. none of these
An ionic bond is the attraction between positively and negatively charged ions in which of these?
Lesson 3 - Now
5. Losing valence electrons can make
some atoms more chemically stable.
6. Metals are good electrical conductors
because they tend to hold onto their
valence electrons very tightly.
Do you agree or disagree?
Chapter Review Menu
Key Concept Summary
Interactive Concept Map
Chapter Review
Standardized Test Practice
The BIG Idea
There are a finite number of elements, and their atoms join together through sharing, transferring, or pooling their electrons to make chemical compounds.
Key Concepts 1
• Electrons with more energy are farther from the atom’s nucleus and are in a higher energy level.
• Atoms with fewer than eight valence electrons gain, lose, or share valence electrons and form stable compounds. Atoms in stable compounds have the same electron arrangement as a noble gas.
Lesson 1: Electrons and Energy
Levels
Key Concepts 2
Lesson 2: Compounds, Chemical
Formulas, and Covalent Bonds
• A compound and the elements it is made from have different chemical and physical properties.
• A covalent bond forms when two nonmetal atoms share valence electrons. Common properties of covalent compounds include low melting points and low boiling points. They are usually gas or liquid at room temperature and poor conductors of electricity.
• Water is a polar compound because the oxygen atom pulls more strongly on the shared valence electrons than the hydrogen atoms do.
Key Concepts 3
• Ionic bonds form when valence electrons from a metal atom transfers to a nonmetal atom.
• An ionic compound is held together by ionic bonds, which are attractions between positively and negatively charged ions.
• A metallic bond forms when valence electrons are pooled among many metal atoms.
Lesson 3: Ionic and Metallic Bonds
Chapter Review – MC1
A. valence electron
B. positive charge
C. chemical bond
D. negative charge
Which term refers to a force that holds two or more atoms together in a compound?
Chapter Review – MC2
A. valence electron
B. nucleus
C. negative electrons
D. proton
Which of these is the outermost electron of an atom that participates in chemical bonding?
Chapter Review – MC3
A. electron
B. proton
C. molecule
D. valence electrons
Which of these is a group of atoms held together by covalent bonding that acts as an independent unit?
Chapter Review – MC4
A. polar molecule
B. covalent bond
C. chemical compound
D. none of these
Which of these describes a chemical bond formed when two atoms share one or more pairs of valence electrons?
Chapter Review – MC5
A. their pooled valence electrons
B. ions
C. charged ions
D. molecules
A metallic bond is a bond formed when many metal atoms share what?
Chapter Review – STP1
A. periodic table
B. energy level
C. atomic number
D. electron dot diagram
Which of these is a model that represents valence electrons in an atom as dots around the element’s chemical symbol?
Chapter Review – STP2
A. reactive
B. chemically unstable
C. chemically stable
D. A and B
Which term describes atoms with unpaired dots in their electron dot diagrams?
Chapter Review – STP3
A. chemical bond
B. chemical formula
C. covalent bond
D. molecule
Which of these describes a group of chemical symbols and numbers that represent the elements and the number of atoms of each element that make up a compound?
Chapter Review – STP4
A. charged ion
B. covalent compound
C. molecule
D. proton
Once an atom gains or loses electrons, it becomes which of these?
Chapter Review – STP5
A. metallic bond
B. ionic bond
C. covalent compound
D. none of these
Which of these refers to the attraction between positively and negatively charged ions in an ionic compound?
