Here are the key points about polar and nonpolar covalent bonds:
- Nonpolar covalent bonds form between atoms with similar electronegativity. Electrons are equally shared. Examples include H2, Cl2, etc.
- Polar covalent bonds form between atoms with different electronegativity. Electrons are unequally shared, resulting in partial positive and negative charges on the atoms. Examples include HCl, H2O.
- Polar molecules are attracted to each other due to their partial charges. They are soluble in polar solvents like water. Nonpolar molecules are not attracted and are soluble in nonpolar solvents like hexane.
- Most bonds have some ionic character based on electrone
For Chem 1:
Significanceof the ELectron in Bonding
The Octet Rule
Lewis Symbol/Structures
Formal Charge
Polyatomic Ions
Types of Bonds (Ionic, Covalent, Coordinate Covalent, Metallic Bonds, Multiple Bonds)
Exceptions to the Octet Rules
Oxidation Number is not included in the class discussion and exam. ;D
For Chem 1:
Significanceof the ELectron in Bonding
The Octet Rule
Lewis Symbol/Structures
Formal Charge
Polyatomic Ions
Types of Bonds (Ionic, Covalent, Coordinate Covalent, Metallic Bonds, Multiple Bonds)
Exceptions to the Octet Rules
Oxidation Number is not included in the class discussion and exam. ;D
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between atoms with opposite charges, or through the sharing of electrons as in the covalent bonds
Chapter 6: Chemical Bonding, Modern Chemistry. This is a working presentation of the notes for this chapter. Meaning that we may or may not cover all of the material here.
chemical bonding and molecular structure class 11sarunkumar31
hybridisation, bonding and antiboding, dipole moment, VSPER theory, Molecular orbital diagram, Phosphorous pentachloride, ionic bond, bond order, bond enthalpy, bond dissociation, sp and sp2hybridisation, hydrogen bonding,electron pair,lone pair repulsion, resonance structure of ozone, how to find electron pair and lone pair, sp3 hybridization of methane.
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between atoms with opposite charges, or through the sharing of electrons as in the covalent bonds
Chapter 6: Chemical Bonding, Modern Chemistry. This is a working presentation of the notes for this chapter. Meaning that we may or may not cover all of the material here.
chemical bonding and molecular structure class 11sarunkumar31
hybridisation, bonding and antiboding, dipole moment, VSPER theory, Molecular orbital diagram, Phosphorous pentachloride, ionic bond, bond order, bond enthalpy, bond dissociation, sp and sp2hybridisation, hydrogen bonding,electron pair,lone pair repulsion, resonance structure of ozone, how to find electron pair and lone pair, sp3 hybridization of methane.
Definition of ionic compounds
Property of ionic compoundIn crystal formSolubility in waterHigh melting and boiling pointConductivity of electricity
Use of ionic compoundUse as dryersUse to make pans
It's very good for SPM students . You have to learn the ionic bond thoroughly. If you understand well you can explain it vividly. For other chemistry notes can email me puterizamrud@gmail.com or facebook Pusat Tuisyen Zamrud .
Chemical bonding xi , dr.mona srivastava , founder masterchemclassesDR MONA Srivastava
Viewers,
This ppt of chemical bonding is designed to give a complete idea and though conceptual extract of the topic for the students of XI to help them understand the basics of chemical bonding in chemistry. Hope it covers all important aspects and points .
Dr Mona Srivastava
Founder-
Masterchemclasses
13 808 PM docs.google.com Covalent Bonding and lonic Bonding study.pdffms12345
10. Identify and discuss the goods oriented remedies of the seller and the buyer 11. ldentify and
discuss the moncy oriented damages of the seller and the buyer 12 identify and discuss the
\"specific performance\" remedies of the seller and buyer.
Solution
Q. 10) Goods oriented remedies of a buyer are as follows
1) When seller became insolvent and buyer wants to recover the goods purchased
In this case , When seller has paid first installment of proice so now he has booked special
property interest in the identified good and seller became insolvent within 10 days following first
receipt of price then to get the good from seller , buyer needs to pay remaining portion of price
and get the product.
2) To sue the buyer.
In this case , when seller is unlawfully not ready to give the product to buyer as buyer has paid in
full price of goods then buyer can sue him.
3) Buyer can enforce security interest in goods
in this case , remedy shall be when buyer fully rejects but he has the product with himself then
buyer has security interest to the extent of any expenses incurred by buyer .
Buyer shall sell the goods and pay the proceeds to seller above the security interest.
Goods oriented remedies of seller are as follows:
1) When buyer breaches
In this case , seller can withhold the delivery of remaining goods
2) When seller comes to know that buyer has become insolvent
In this case , seller will stop the delivery of goods till the time goods are in transit.
3) When buyer breaches and goods are in process
in this case , seller shall stop the production and unfinished goods shall be sold as scrap so the
damages of seller can be recovered
Q 11) Money oriented remedies of buyer are as follows
1) When seller breaches regarding payment made
in this case , buyer should recover as much price he has already paid and then return the goods.
2) when seller breaches then buyer should cover
in this case , buyer can buy substitute while acting in good faith and then try to cover the
expenses incurred. If buyer doesnt cover then he will not be able to cover his damages
3) When seller breaches then buyer needs to cover damages for non delivery
in this case , damages = (contract price -market price ) + expenses incurred.
Money oriented remedies of seller are as follows
1) When buyer breaches then
in this case , seller shall resell the goods to recover damages in good faith and evn seller may
give notice to buyer for breach of contract
2) When buyer breaches regarding non acceptance of goods
in this case , seller shall recover damages as the difference between the market price and place of
sell plus any expenses incurred.
3) When buyer breaches regarding price to be paid
in this case , seller shall recover the price by conforming goods are lost and damaged after risk of
loss is transfered to buyer
Specific performance remedies of the buyer are as follows
1) When seller breaches then buyer may cancel
in this case , buyer can cancel by repudiating the contract.
2) when sel.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
Normal Labour/ Stages of Labour/ Mechanism of LabourWasim Ak
Normal labor is also termed spontaneous labor, defined as the natural physiological process through which the fetus, placenta, and membranes are expelled from the uterus through the birth canal at term (37 to 42 weeks
This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...Levi Shapiro
Letter from the Congress of the United States regarding Anti-Semitism sent June 3rd to MIT President Sally Kornbluth, MIT Corp Chair, Mark Gorenberg
Dear Dr. Kornbluth and Mr. Gorenberg,
The US House of Representatives is deeply concerned by ongoing and pervasive acts of antisemitic
harassment and intimidation at the Massachusetts Institute of Technology (MIT). Failing to act decisively to ensure a safe learning environment for all students would be a grave dereliction of your responsibilities as President of MIT and Chair of the MIT Corporation.
This Congress will not stand idly by and allow an environment hostile to Jewish students to persist. The House believes that your institution is in violation of Title VI of the Civil Rights Act, and the inability or
unwillingness to rectify this violation through action requires accountability.
Postsecondary education is a unique opportunity for students to learn and have their ideas and beliefs challenged. However, universities receiving hundreds of millions of federal funds annually have denied
students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
Thinking of getting a dog? Be aware that breeds like Pit Bulls, Rottweilers, and German Shepherds can be loyal and dangerous. Proper training and socialization are crucial to preventing aggressive behaviors. Ensure safety by understanding their needs and always supervising interactions. Stay safe, and enjoy your furry friends!
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
A review of the growth of the Israel Genealogy Research Association Database Collection for the last 12 months. Our collection is now passed the 3 million mark and still growing. See which archives have contributed the most. See the different types of records we have, and which years have had records added. You can also see what we have for the future.
How to Add Chatter in the odoo 17 ERP ModuleCeline George
In Odoo, the chatter is like a chat tool that helps you work together on records. You can leave notes and track things, making it easier to talk with your team and partners. Inside chatter, all communication history, activity, and changes will be displayed.
Digital Artefact 1 - Tiny Home Environmental Design
Chem unit 7 presentation
1.
2. Main Ideas
Atoms gain stability when they share
electrons and form covalent bonds.
Specific rules are used when naming
binary molecular compounds, binary
acids, and oxyacids.
Structural formulas show the relative
positions of atoms within a molecule
3. Main Ideas
The VSEPR model is used to determine
molecular shape.
A chemical bond’s character is related to
each atom’s attraction for the electrons in
the bond.
4.
5. Objectives
Describe the formation of single, double, and
triple covalent bonds by applying the octet
rule.
Contrast sigma and pi bonds.
Relate the strength of a covalent bond to its
bond length and bond dissociation energy.
6. Why do atoms bond?
Atoms gain stability when they share electrons
and form covalent bonds.
Lower energy states make an atom more
stable.
Gaining or losing electrons makes atoms
more stable by forming ions with noble-gas
electron configurations.
Sharing valence electrons with other atoms
also results in noble-gas electron
7. Covalent Bond
Atoms in non-ionic compounds share electrons.
The chemical bond that results from sharing
electrons is a covalent bond.
A molecule is formed when two or more
atoms bond.
8. Diatomic Molecules
Diatomic molecules exist because two-atom
molecules are more stable than single
atoms.
Examples: H2, N2, O2, F2, Cl2, Br2, I2
9. Why do atoms bond?
The most stable
arrangement of atoms
exists at the point of
maximum net attraction,
where the atoms bond
covalently and form a
molecule.
10. Single Covalent Bonds
When only one pair of electrons is shared, the result
is a single covalent bond.
The figure shows two hydrogen atoms forming a
hydrogen molecule with a single covalent bond,
resulting in an electron configuration like helium.
11. Single Covalent Bonds
Also called Sigma Bond – represented by δ – forms
when valence atomic orbitals overlap and share
localized electrons.
12. Single Covalent Bonds
In a Lewis structure, dots or a line are used to
symbolize a single covalent bond.
The halogens—the group 17 elements—
have 7 valence electrons and form single
covalent bonds with atoms of other non-
metals
Example: HF
13. Single Covalent Bonds
Atoms in group 16 can share two electrons
and form two covalent bonds.
Water is formed from one oxygen with two
hydrogen atoms covalently bonded to it .
14. Single Covalent Bonds
Atoms in group 15 form three single covalent
bonds, such as in ammonia.
15. Single Covalent Bonds
Atoms of group 14 elements form four single
covalent bonds, such as in methane.
16. Single Covalent Bonds
Sigma bonds are single covalent bonds.
Sigma bonds occur when the pair of shared
electrons is in an area centered between the
two atoms.
17. Multiple Covalent Bonds
Double bonds form when two pairs of electrons
are shared between two atoms.
Triple bonds form when three pairs of electrons
are shared between two atoms.
18. Multiple Covalent Bonds
A multiple covalent bond consists of one sigma
bond and at least one pi bond
The pi bond is formed when parallel orbitals
overlap and share electrons.
19. Strength of Covalent
Bonds
Bond Length is the distance between two
bonded nuclei at the position of maximum
attraction.
The strength depends on the distance
between the two nuclei, or bond length
As length increases, strength decreases
21. Strength of Covalent
Bonds
The amount of energy required to break a bond
is called the bond dissociation energy.
The shorter the bond length, the greater the
energy required to break it.
22. Strength of Covalent
Bonds
An endothermic reaction is one where a
greater amount of energy is required to
break a bond in reactants than is released
when the new bonds form in the products.
An exothermic reaction is one where more
energy is released than is required to break
the bonds in the initial reactants.
23. Question 1
What does a triple bond consists of?
A. three sigma bonds
B. three pi bonds
C. two sigma bonds and one pi bond
D. two pi bonds and one sigma bond
24. Question 2
Covalent bonds are different from ionic bonds
because:
A. atoms in a covalent bond lose electrons to another
atom
B. atoms in a covalent bond do not have noble-gas
electron configurations
C. atoms in a covalent bond share electrons with
another atom
D. atoms in covalent bonds gain electrons from another
atom
27. Objectives
Translate molecular formulas into
binary molecular compound names.
Define binary and oxyacids.
Name acidic solutions
28. Naming Binary Molecular
Compounds
1. The first element is always named
first using the entire element name.
2. The second element is named using
its root and adding the suffix –ide.
29. Naming Binary Molecular
Compounds
3. Prefixes are used to indicate the
number of atoms of each element in a
compound.
30. Naming Binary Molecular
Compounds
Many compounds were discovered and
given common names long before the
present naming system was developed
(water, ammonia, hydrazine, nitric
oxide)
31. Acids
Acids produce H+ atoms in an aqueous
solution. Two common types are binary and
oxyacids.
Binary Acids have a hydrogen and one other
element.
Examples: HF, HCl
Exception: HCN: hydrocyanic acid
Oxyacids are acids that contain an oxygen
Examples: HNO3, H3PO4
32. Naming Binary Acids
1. The first word has the prefix hydro-
followed by the root of the element plus
the suffix –ic.
2. The second word is always acid
(hydrochloric acid is HCl in water)
Examples:
33. Naming Oxyacids
1. Identify the oxyanion present.
The first word is the root of the oxyanion and
the prefix per- or hypo- if it is part of the
name
plus the suffix -ic if the anion ends in
-ate
plus the suffix -ous if the oxyanion ends in -
ite.
35. Naming Acids
An acid, whether a binary acid or an
oxyacid, can have a common name in
addition to its compound name.
36. Naming Acids
The name of a molecular compound
reveals its composition and is important
in communicating the nature of the
compound.
37. Writing Formulas from
Names
Use the prefixes to give you the
numbers of atoms present in a
compound.
Remember that all binary and oxyacids
contain hydrogen. A prefix will tell you
the quantity of hydrogen in the formula,
you must balance the charge of your
oxyanion.
39. Question 1
Give the binary molecular name for
water (H2O).
A. dihydrogen oxide
B. dihydroxide
C. hydrogen monoxide
D. dihydrogen monoxide
40. Question 2
Give the name for the molecule HClO4.
A. perchloric acid
B. chloric acid
C. chlorous acid
D. hydrochloric acid
41. Practice Problems and
Homework
CALM 7:2
p249 #14-18
p251 #19-24
p251-2 #25-30, 31-36
42.
43. Objectives
List the basic steps used to draw Lewis
structures.
Explain why resonance occurs, and
identify resonance structures.
Identify three exceptions to the octet
rule, and name molecules in which
these exceptions occur.
44. Structural Formula
A structural formula uses letter symbols and
bonds to show relative positions of atoms.
Atoms within a polyatomic ion are covalently
bonded.
45. Structural Formulas
Rules for Drawing Lewis Structures
1. Predict the location of certain atoms.
The atom with the lowest electronegativity (except
H) is typically in the center.
2. Determine the number of electrons available for
bonding.
Add up all the valence electrons of the atoms that
make up the compound
46. Structural Formulas
Rules for Drawing Lewis Structures
3. Determine the number of bonding pairs.
Take the number of total valence electrons and
divide by two.
4. Place the bonding pairs.
47. Structural Formulas
Rules for Drawing Lewis Structures
5. Determine the number of bonding pairs
remaining.
Subtract bonded electrons (step 4) from available
electrons (step 3)
This is the number of valence electrons assigned
as lone pairs
Place lone pairs around the terminal atoms to satisfy
the octet rule, except H
Remaining electrons ‘belong’ to the central atom.
48. Structural Formulas
Rules for Drawing Lewis Structures
6. Determine whether the central atom satisfies the
octet rule
If the central atom does not have 4 pairs of
electrons around it, use remaining electrons to
form double or triple bonds.
C,N,O and S often form multiple bonds.
49. Resonance Structures
Resonance is a condition that occurs when more
than one valid Lewis structure can be written for a
molecule or ion.
This figure shows three correct ways to draw the
structure for (NO3)-.
50. Resonance Structures
The molecule behaves as though it has only
one structure.
The bond lengths are identical to
each other and intermediate
between single and double
covalent bonds.
51. Exceptions to the Octet
Rule
Some molecules do not obey the octet rule
1. A small group of molecules might have an
odd number of valence electrons.
NO2 has five valence electrons from nitrogen
and 12 from oxygen and cannot form an exact
number of electron pairs.
52. Exceptions to the Octet
Rule
2. Suboctets and coordinate covalent bonds:
A few compounds form stable configurations with
less than 8 electrons around the atom—a suboctet.
A coordinate covalent bond forms when one atom
donates both of the electrons to be shared with an
atom or ion that needs two electrons.
53. Exceptions to the Octet
Rule
3. A third group of compounds has central
atoms with more than eight valence
electrons, called an expanded octet.
Elements in period 3 or higher have a
d-orbital and can form more than four
covalent bonds.
54. Question 1
What is it called when one or more
correct Lewis structures can be
drawn for a molecule?
A. suboctet
B. expanded octet
C. expanded structure
D. resonance
55. Question 2
Where do atoms with expanded octets
occur?
A. transition metals
B. noble gases
C. elements in period 3 or higher
D. elements in group 3 or higher
58. Objectives
Summarize the VSEPR bonding
theory.
Predict the shape of, and the bond
angles in, a molecule.
Define hybridization.
59. VSEPR Model
The shape of a molecule determines many of
its physical and chemical properties.
Molecular geometry (shape) can be
determined with the Valence Shell Electron
Pair Repulsion model, or VSEPR model
which minimizes the repulsion of shared
and unshared atoms around the central
atom.
60. VSEPR Model
Electron pairs repel each other and
cause molecules to be in fixed positions
relative to each other.
Unshared electron pairs also determine
the shape of a molecule.
Electron pairs are located in a molecule
as far apart as they can be.
61. Hybridization
Hybridization is a process in which atomic
orbitals mix and form new, identical hybrid
orbitals.
Carbon often undergoes hybridization,
which forms an sp3 orbital formed from
one s orbital and three p orbitals.
Lone pairs also occupy hybrid orbitals
66. Bond Angles
Bond Angle- the angle formed between
two terminal atoms and a central atom.
Electron pairs, shared and unshared,
in a molecule repel one another and
create fixed angles between atoms in a
molecule. Unshared electron pairs
cause more repulsion
67. Question 1
The two lone pairs of electrons on a water molecule do
what to the bond angle between the hydrogen
atoms and the oxygen atom?
A. They attract the hydrogen atoms and increase the
angle greater than 109.5°.
B. They occupy more space and squeeze the hydrogen
atoms closer together.
C. They do no affect the bond angle.
D. They create resonance structures with more than one
correct angle.
68. Question 2
The sp3 hybrid orbital in CH4 has what
shape?
A. linear
B. trigonal planar
C. tetrahedral
D. octahedral
71. Objective
Describe how electronegativity is used
to determine bond type.
Compare and contrast polar and
nonpolar covalent bonds and polar and
nonpolar molecules.
Generalize about the characteristics of
covalently bonded compounds.
72. Electron Affinity, Electronegativity
and Bond Character
Electron affinity measures the tendency of an
atom to accept an electron.
Noble gases are not listed because they
generally do not form compounds.
Similar to Electronegativity – electron love! –
the relative ability of an atom to attract
electrons in a chemical bond.
73. Electron Affinity, Electronegativity
and Bond Character
This table lists the character and type of
chemical bond that forms with
differences in electronegativity.
74. Electron Affinity, Electronegativity
and Bond Character
Unequal sharing of electrons results in
a polar covalent bond.
Bonding is often not clearly ionic or
covalent
75. Electron Affinity, Electronegativity
and Bond Character
bonds are never completely ionic or completely
covalent. The character of the bond (more covalent
or more ionic) is determined by the differences in
electronegativities of the atoms that are bonding.
76. Covalent Bonds
Covalently bonded molecules are either
polar or non-polar.
An electronegativity difference of 1.70
is considered to be 50% ionic and 50%
covalent.
77. Nonpolar Covalent
Nonpolar covalent bonds have electrons that
are equally shared between the two atoms.
Electronegativites are the same or very
similar
Diatomic molecules
Nonpolar molecules are not attracted by an
electric field
78. Polar Covalent Bonds
Polar covalent bonds form when there is
unequal sharing of electrons due to a
difference in electronegativities of the atoms
bonded.
Electrons spend more time around one atom
than another resulting in partial charges at the
ends of the bond called a dipole.
79. Polar Covalent Bonds
Polar molecules align with an electric
field
Compare water and CCl4
Both bonds are polar, but only water is
a polar molecule because of the shape
of the molecule.
80. Polar Covalent Bonds
The electric charge on a CCl4 molecule
measured at any distance from the center of the
molecule is identical to the charge measured at
the same distance on the opposite side.
81. Solubility
Solubility is the property of a substance’s
ability to dissolve in another substance.
Polar molecules and ionic substances
are usually soluble in polar substances.
Non-polar molecules dissolve only in
non-polar substances.
82. Molecular Polarity
Molecular polarity (Dipole) - differences in
electronegativities causes polarity in molecules
by the position of electron densities.
δ(delta) partial charge – is used to show polarity
charge on molecules.
Dipole moment – difference in electronegativities
that cause molecular polarity of dipole.
83. Properties of Covalent
Compounds
Non-polar molecules exhibit a weak dispersion force,
or induced dipole.
The force between two oppositely charged ends of
two polar molecules is a dipole-dipole force.
A hydrogen bond is an especially strong dipole-dipole
force between a hydrogen end of one dipole and a
fluorine, oxygen, or nitrogen atom on another dipole.
84. Properties of Covalent
Molecules
Covalent bonds between atoms are strong,
but attraction forces between molecules are
weak.
The weak attraction forces are known as
van der Waals forces.
The forces vary in strength but are weaker
than the bonds in a molecule or ions in an
ionic compound.
85. Properties of Covalent
Compounds
Many physical properties are due to intermolecular
forces.
Weak forces result in the relatively low melting
and boiling points of molecular substances.
Many covalent molecules are relatively soft solids.
Molecules can align in a crystal lattice, similar to
ionic solids but with less attraction between
particles.
86. Properties of Covalent
Compounds
Solids composed of only atoms
interconnected by a network of covalent
bonds are called covalent network
solids.
Quartz and diamonds are two common
examples of network solids.
87. Question 1
The force between water molecules is
what kind of intermolecular force?
A. induced dipole
B. hydrogen bond
C. sigma bond
D. partial dipole
88. Question 2
What kind of bond occurs within a
molecule with unequal sharing of
electron pairs?
A. ionic bond
B. sigma bond
C. non-polar covalent bond
D. polar covalent bond
90. Study Guide
Covalent bonds form when atoms share one or more
pairs of electrons.
Sharing one pair, two pairs, and three pairs of
electrons forms single, double, and triple covalent
bonds, respectively.
Orbitals overlap directly in sigma bonds. Parallel
orbitals overlap in pi bonds.
91. Study Guide
A single covalent bond is a sigma bond but multiple
covalent bonds are made of both sigma and pi
bonds.
Bond length is measured nucleus-to-nucleus.
Bond dissociation energy is needed to break
a covalent bond.
Names of covalent molecular compounds include
prefixes for the number of each atom present. The
final letter of the prefix is dropped if the element
name begins with a vowel.
92. Study Guide
Molecules that produce H+ in solution are acids.
Binary acids contain hydrogen and one other
element. Oxyacids contain hydrogen and an
oxyanion.
Resonance occurs when more than one valid Lewis
structure exists for the same molecule.
Exceptions to the octet rule occur in some
molecules.
VSEPR model theory states that electron pairs repel
each other and determine both the shape of and
93. Study Guide
Hybridization explains the observed shapes of
molecules by the presence of equivalent hybrid
orbitals
The electronegativity difference determines the
character of a bond between atoms.
Polar bonds occur when electrons are not shared
equally forming a dipole.
The spatial arrangement of polar bonds in a
molecule determines the overall polarity of a
molecule.
94. Study Guide
Molecules attract each other by weak intermolecular
forces. In a covalent network solid, each atom is
covalently bonded to many other atoms.