Chapter 10- Chemical Bonding

Chapter 10- Chemical Bonding

Multiple Select

If the amplitude increases, the energy of the wave:

• increases

• decreases

• stays the same

Multiple Choice

What is a wavelength?

• How many waves pass a certain point?

• The distance from one wave crest to another

• The entire length of a wave

Multiple Choice

Which wave has a greater frequency?

• A
• B

Multiple Choice

If a wave has a greater frequency, what happens to the wavelength?

• increases

• decreases

• stays the same

Multiple Choice

Which letter represents amplitude?

• A
• B
• C
• D

Multiple Choice

Which letter represents wavelength?

• A
• B
• C
• D

Multiple Choice

What does the arrow in the picture represent?

• wavelength

• echolocation

• amplitude

• peak

Multiple Choice

How many protons are in the element, "Sodium?"

• 23
• 11
• 13
• 14

Multiple Choice

an atom with atomic number 6 would have how many protons 

• 6
• 12
• 3
• cannot be determined 

Multiple Choice

What is the correct set of quantum numbers for the last entering electron of magnesium?

• n=2 l=0 ml=0 ms=-1/2

• n=3 l=0 ml=0 ms=-1/2

• n=3 l=1 ml=-1 ms=+1/2

• n=3 l=0 ml=0 ms=+1/2

Multiple Choice

What orbital does the last entering electron of chlorine belong?

• 2s²

• 2p⁵

• 3p⁵

• 4d⁵

Multiple Choice

What is the correct electron configuration of silicon?

• 1s² 2s² 2p⁶ 3p⁴

• 1s² 2s² 3p⁶ 4s² 3d²

• 1s² 2s² 2p⁶ 3s² 3p²

• 1s² 2s² 3p⁶ 3s² 4p²

Multiple Choice

What type of sublevel has the this shape?

• s

• p

• d

• f

Multiple Choice

Which of the following is the correct Lewis dot structure for the molecule fluorine (F₂)?

• A
• B
• C
• D

Multiple Choice

Which is the correct molecular structure for carbon dioxide?

Multiple Choice

How many total valence electrons are participating in bonding in the molecule above?

• 8

• 4

• 2

• 3

Multiple Choice

CO₂ has how many lone pairs?

• 0

• 1

• 2

• 3

• 4

Multiple Choice

NH₃ has how many lone pairs?

• 0

• 1

• 2

• 3

Second part...

By Luis Bello

Octet Rule

The octet rule states that atoms tend to form compounds in ways that give them eight valence electrons and thus the electron configuration of a noble gas. 

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An exception to an octet of electrons is in the case of the first noble gas, helium, which only has two valence electrons. 

​

• Atoms form compounds in ways that give them eight valence electrons.

• Metals tend to lose electrons to achieve this configuration.

• Nonmetals tend to gain electrons to achieve this configuration.

​

Cation Formation

Cations are the positive ions formed by the loss of one or more electrons.  The most commonly formed cations of the representative elements are those that involve the loss of all of the valence electrons.  Consider the alkali metal sodium (Na). 

It has one valence electron in the third principal energy level.  Upon losing that electron, the sodium ion now has an octet of electrons from the second principal energy level.

• Cations form when an atom loses one or more electrons.

• The resulting cation has the electron configuration of the noble gas atom in the row above it in the periodic table.​

Anion Formation

Anions are the negative ions formed from the gain of one or more electrons.  When nonmetal atoms gain electrons, they often do so until their outermost principal energy level achieves an octet.  This process is illustrated below for the elements fluorine, oxygen, and nitrogen.

​

• Anions are negative ions formed by accepting electrons.

• The outermost principal energy level usually is an octet.

​

​VSEPR Chart | Valence Shell Electron Pair Repulsion Theory

WHAT IS VSEPR THEORY?

​

The valence shell electron pair repulsion (VSEPR) theory is a model used to predict 3-D molecular geometry based on the number of valence shell electron bond pairs among the atoms in a molecule or ion.

This model assumes that electron pairs will arrange themselves to minimize repulsion effects from one another. In other words, the electron pairs are as far apart as possible.

​VSEPR SHAPES

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The VSEPR model is useful for predicting and visualizing molecular structures.

​

The structures are linear, trigonal planar, angled, tetrahedral, trigonal pyramidal, trigonal bipyramidal, disphenoidal (seesaw), t-shaped, octahedral, square pyramidal, square planar, and pentagonal bipyramidal.

​Metallic Bond

​

Pure metals are crystalline solids, but unlike ionic compounds, every point in the crystal lattice is occupied by an identical atom. 

The electrons in the outer energy levels of metal are mobile and capable of drifting from one metal atom to another. 

This means that the metal is more properly viewed as an array of positive ions surrounded by a sea of mobile valence electrons. 

Electrons that are capable of moving freely throughout the empty orbitals of the metallic crystal are called delocalized electrons. 

A metallic bond is the attraction of the stationary metal cations to the surrounding mobile electrons.

​

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Multiple Choice

What is the number of electrons that an atom needs to be stable?

• 2
• 8
• 10
• 12

Multiple Choice

What type of bond shares a pair of electrons?

• atomic
• hydrogen
• covalent
• ionic

Multiple Choice

Unequal sharing of a pair of electrons within a bond is

• ionic
• polar covalent
• nonpolar covalent
• hydrogen

Multiple Choice

Why do elements share electrons at all?

• They want to be stable
• They are greedy and always want more
• Positive and negative forces attract
• The electrons just do what they want

Multiple Choice

Hydrogen bonding occurs between 

• Hydrogen and zinc
• Hydrogen and oxygen
• Hydrogen and lithium
• Hydrogen and helium

Multiple Choice

Which of the following bonds has an atom that steals electrons from another atom?

• ionic
• polar covalent
• nonpolar covalent
• hydrogen

Multiple Choice

According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?

• Pairs of valence electrons
• Inner shell electrons
• Mobile Electrons
• Electrons closest to the nucleus

Multiple Choice

Which of the following molecular shapes would have a bond angle of 180 Degrees?

• Bent
• Trigonal Planar
• Tetrahedral
• Linear

Multiple Choice

What is the measure of a tetrahedral bond angle?

• 90 Degrees
• 109.5 Degrees
• 120 Degrees
• 180 Degrees

Multiple Choice

Which molecule would have this shape?

• BF₃
• CH₄
• PCl₅
• CO₂

Multiple Choice

The bond angle for a trigonal planar molecule is 

• 90 Degrees
• 109.5 Degrees
• 120 Degrees
• 180 Degrees

Multiple Choice

The ------ model helps predict the shape of a molecule.

• VESPR

• Electron

• Lewis

Multiple Choice

The ability of the metal to be drawn into wires.

• Moving Electrons

• Malleability

• Ductility

Multiple Choice

What are charged particles that form when atoms gain or lose electrons?

• Particle Atoms

• Ions

• Atomic Ions

• Bonds

Multiple Choice

What do you call a bond that forms when electrons are transferred from one atom to another?

• Compound Bond

• Ionic Bond

• Crystal Bond

• Atom Bond