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Questions and Answers
What characterizes a double bond between two atoms?
What characterizes a double bond between two atoms?
Which of the following is a property of ionic compounds?
Which of the following is a property of ionic compounds?
According to the VSEPR Theory, what primarily determines the shape of a molecule?
According to the VSEPR Theory, what primarily determines the shape of a molecule?
What type of bond is formed by the overlap of two orbitals head-on?
What type of bond is formed by the overlap of two orbitals head-on?
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Which characteristic is NOT typical of covalent compounds?
Which characteristic is NOT typical of covalent compounds?
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What is the three-dimensional arrangement of ions in Sodium Chloride called?
What is the three-dimensional arrangement of ions in Sodium Chloride called?
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How many chloride ions surround each sodium ion in Sodium Chloride?
How many chloride ions surround each sodium ion in Sodium Chloride?
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What is the total charge contributed by aluminium in Aluminium Oxide?
What is the total charge contributed by aluminium in Aluminium Oxide?
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To obtain a neutral compound of Aluminium Oxide, what is the lowest common multiple of the charges of Aluminium and Oxygen?
To obtain a neutral compound of Aluminium Oxide, what is the lowest common multiple of the charges of Aluminium and Oxygen?
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Which groups of elements typically form ionic compounds?
Which groups of elements typically form ionic compounds?
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What distinguishes the bonding in PH3 from that in H2O, NH3, and HCl?
What distinguishes the bonding in PH3 from that in H2O, NH3, and HCl?
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Which hydrides exhibit hydrogen bonding between their molecules?
Which hydrides exhibit hydrogen bonding between their molecules?
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What effect does hydrogen bonding have on the boiling point of H2O and NH3?
What effect does hydrogen bonding have on the boiling point of H2O and NH3?
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How does the symmetry of BCl3 affect its polarity?
How does the symmetry of BCl3 affect its polarity?
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What is the molecular shape of PH3 and how does it arise from electron-pair repulsion?
What is the molecular shape of PH3 and how does it arise from electron-pair repulsion?
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What type of bonding is characterized by temporary dipoles that induce attraction between non-polar molecules?
What type of bonding is characterized by temporary dipoles that induce attraction between non-polar molecules?
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Which type of intermolecular force is considered stronger than Van der Waals forces but weaker than ionic bonds?
Which type of intermolecular force is considered stronger than Van der Waals forces but weaker than ionic bonds?
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What primarily determines the strength of Van der Waals forces in a molecule?
What primarily determines the strength of Van der Waals forces in a molecule?
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Which atoms, when bonded to hydrogen, can create strong hydrogen bonds?
Which atoms, when bonded to hydrogen, can create strong hydrogen bonds?
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Which intermolecular force is primarily responsible for the higher boiling points of polar molecules compared to non-polar molecules?
Which intermolecular force is primarily responsible for the higher boiling points of polar molecules compared to non-polar molecules?
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What occurs when the partial positive charge of a hydrogen atom bonded to an electronegative atom is attracted to another electronegative atom?
What occurs when the partial positive charge of a hydrogen atom bonded to an electronegative atom is attracted to another electronegative atom?
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What type of forces exist between molecules characterized by permanent dipoles?
What type of forces exist between molecules characterized by permanent dipoles?
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Which relationship between Van der Waals forces and molecular size is true?
Which relationship between Van der Waals forces and molecular size is true?
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What is the reason that water is a polar molecule?
What is the reason that water is a polar molecule?
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How does the electronegativity difference define the type of bonding in a compound?
How does the electronegativity difference define the type of bonding in a compound?
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What happens when a polar liquid is exposed to a charged plastic rod?
What happens when a polar liquid is exposed to a charged plastic rod?
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Which of the following is a characteristic of a non-polar liquid?
Which of the following is a characteristic of a non-polar liquid?
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What occurs to ionic substances like sodium chloride when dissolved in water?
What occurs to ionic substances like sodium chloride when dissolved in water?
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What type of covalent bond is indicated by an electronegativity difference of 0.35?
What type of covalent bond is indicated by an electronegativity difference of 0.35?
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What bonding characteristics are associated with ionic compounds?
What bonding characteristics are associated with ionic compounds?
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Which statement about intramolecular bonding is true?
Which statement about intramolecular bonding is true?
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What is the strongest form of intermolecular force?
What is the strongest form of intermolecular force?
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How many sigma and pi bonds are present in a molecule of nitrogen?
How many sigma and pi bonds are present in a molecule of nitrogen?
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What defines electronegativity?
What defines electronegativity?
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Which molecule has hydrogen bonding between its molecules?
Which molecule has hydrogen bonding between its molecules?
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What is the bond angle in a molecule of ammonia (NH3)?
What is the bond angle in a molecule of ammonia (NH3)?
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Why does hydrogen have a lower boiling point compared to oxygen?
Why does hydrogen have a lower boiling point compared to oxygen?
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What describes intramolecular bonding?
What describes intramolecular bonding?
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How can a molecule with polar bonds be non-polar?
How can a molecule with polar bonds be non-polar?
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Study Notes
Chemical Bonding
- A compound is a substance made of two or more different elements combined chemically.
- Attractive forces hold atoms together in a compound, called chemical bonds.
The Octet Rule
- Atoms tend to gain, lose, or share electrons to achieve an electron arrangement with eight electrons in their outermost energy level (octet rule).
- Noble gases are unreactive because they already have a stable octet.
- Elements in the same group have similar properties.
Exceptions to the Octet Rule
- Transition metals frequently do not follow the octet rule.
- Hydrogen, lithium, and beryllium tend to achieve two electrons in their outermost shell instead of eight.
Ionic Bonding
- An ion is a charged atom or group of atoms.
- Atoms gain or lose electrons to have the electron configuration of a noble gas.
- Atoms in group 1 lose one electron, forming a positive ion.
- Atoms in group 2 lose two electrons, forming a positive ion.
- Atoms in group 6 or 7 gain electrons, forming a negative ion (anion).
- Ionic bonds result from the attraction between oppositely charged ions.
- Ionic compounds form crystal lattices.
How to Write Formulas for Ionic Compounds
- Chemical formulas show the atoms in a compound and their quantities.
- Ionic compounds are typically composed of metals in groups 1 and 2 and nonmetals in groups 6 and 7.
- The overall charge of an ionic compound must be zero; the charges on the ions balance.
Dot and Cross Diagrams
- Used to represent the bonding in simple compounds.
- Dots represent the outer electrons of one atom.
- Crosses represent the outer electrons of another atom.
- Arrows show the transfer of electrons.
Sodium Chloride Crystal Structure
- X-ray studies reveal the arrangement of ions in a crystal lattice.
- Sodium chloride has a cubic structure.
- Each sodium ion is surrounded by 6 chloride ions, and vice-versa.
Common Polyatomic Ions
- Memorize common polyatomic ions or groups of atoms which carry a net charge.
Transition Metals
- Transition metals have variable valencies (charges).
- Predicting charges for transition metal compounds requires knowledge of common charges for these metals.
Covalent Bonding
- Atoms share electrons to achieve a stable electron configuration.
- Bond pairs are pairs of electrons shared between atoms.
- Lone pairs are electron pairs that are not involved in bonding.
- Covalent bonds can be nonpolar or polar covalent.
Molecules
- A molecule is a group of atoms bonded together.
- Molecules can be represented by dot and cross diagrams.
Sigma and Pi bonds
- Sigma bonds: formed by head-on overlap of orbitals.
- Pi bonds: formed by sideways overlap of p orbitals.
- Single bonds are only sigma bonds.
- Double bonds have one sigma and one pi bond.
- Triple bonds have one sigma and two pi bonds.
Electronegativity
- Electronegativity measures an atom's ability to attract electrons in a bond.
- Differences in electronegativities determine bond polarity (polar or nonpolar).
- Significant difference in electronegativity (greater than 1.7) indicates ionic bonding.
- Smaller differences (less than 1.7) suggest covalent or polar covalent bonding.
Types of Intermolecular Forces
- Van der Waals: weak forces between all molecules (including nonpolar).
- Dipole-dipole: attractive forces between polar molecules.
- Hydrogen bonding: strong type of dipole-dipole force between molecules containing hydrogen bonded to nitrogen, oxygen, or fluorine.
Properties of Ionic and Covalent Compounds
- Ionic compounds: high melting/boiling points, hard and brittle, conduct electricity in molten or dissolved states.
- Covalent compounds: low melting/boiling points, varying physical states, usually soft, do not conduct electricity.
Shapes of Molecules
- Molecular shape is critical in determining properties.
- Used Valence Shell Electron Pair Repulsion (VSEPR) Theory to determine molecular shapes.
Prediction of Intermolecular Forces
- Consider bond polarity and types of atoms involved to predict the intermolecular forces.
Predicting Bond Type
- Large electronegativity differences predict ionic bonding.
- Smaller differences predict covalent bonding.
- Moderate differences predict polar covalent bonding.
Exam Questions
- Students should study example questions and practice applying concepts.
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Description
Explore the essential concepts of chemical bonding, including the formation of compounds and the significance of the octet rule in achieving electron stability. Delve into exceptions and the mechanisms of ionic bonding. This quiz will test your understanding of these fundamental chemistry topics.
