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Questions and Answers
Considering periodic trends, which of the following elements would likely exhibit the lowest first ionization energy?
Considering periodic trends, which of the following elements would likely exhibit the lowest first ionization energy?
- Phosphorus (P)
- Cesium (Cs) (correct)
- Oxygen (O)
- Fluorine (F)
A compound is found to have a very high melting point and conducts electricity only when dissolved in water. What type of bonding is most likely present?
A compound is found to have a very high melting point and conducts electricity only when dissolved in water. What type of bonding is most likely present?
- Covalent network bonding
- Polar covalent bonding
- Metallic bonding
- Ionic bonding (correct)
Which of the following Lewis structures correctly represents the bonding in sulfur dioxide ($SO_2$), considering formal charge minimization and the octet rule?
Which of the following Lewis structures correctly represents the bonding in sulfur dioxide ($SO_2$), considering formal charge minimization and the octet rule?
- O=S=O (both S-O bonds are double bonds)
- O=S-O (one S-O bond is a double bond, one is a single bond, sulfur has one lone pair, and resonance structures exist) (correct)
- O≡S-O (one S-O bond is a triple bond, one is a single bond, sulfur has no lone pairs)
- O-S-O (both S-O bonds are single bonds, sulfur has two lone pairs)
Which of the following molecules is nonpolar despite containing polar bonds?
Which of the following molecules is nonpolar despite containing polar bonds?
Considering molecular orbital theory, which diatomic species is predicted to have the highest bond order and, therefore, the shortest bond length?
Considering molecular orbital theory, which diatomic species is predicted to have the highest bond order and, therefore, the shortest bond length?
Considering the principles of resonance, how does the stability of a molecule with resonance structures compare to a hypothetical molecule with a single, fixed structure?
Considering the principles of resonance, how does the stability of a molecule with resonance structures compare to a hypothetical molecule with a single, fixed structure?
Given the relationship between bond order, bond length, and bond strength, how would you rank the carbon-carbon bonds in ethane (C₂H₆), ethene (C₂H₄), and ethyne (C₂H₂) in terms of their bond energies, from strongest to weakest?
Given the relationship between bond order, bond length, and bond strength, how would you rank the carbon-carbon bonds in ethane (C₂H₆), ethene (C₂H₄), and ethyne (C₂H₂) in terms of their bond energies, from strongest to weakest?
If a molecule has a central atom with sp² hybridization, one lone pair, and two bonded atoms, what is its molecular geometry and how does the lone pair affect the bond angle between the bonded atoms?
If a molecule has a central atom with sp² hybridization, one lone pair, and two bonded atoms, what is its molecular geometry and how does the lone pair affect the bond angle between the bonded atoms?
Assuming a diatomic molecule is formed between two elements with significantly different electronegativities, which of the following statements accurately describes the distribution of electron density and the resulting bond polarity?
Assuming a diatomic molecule is formed between two elements with significantly different electronegativities, which of the following statements accurately describes the distribution of electron density and the resulting bond polarity?
Considering the trends in the periodic table, which element is the most likely to exhibit metallic properties, including high electrical conductivity and malleability, and readily form positive ions?
Considering the trends in the periodic table, which element is the most likely to exhibit metallic properties, including high electrical conductivity and malleability, and readily form positive ions?
Flashcards
Electronegativity
Electronegativity
The ability of an atom to attract electrons in a chemical bond.
Ionic Bond
Ionic Bond
Electrostatic attraction between oppositely charged ions, typically between a metal and a nonmetal.
Covalent Bond
Covalent Bond
A bond formed by sharing electrons between two atoms.
Lewis Structure
Lewis Structure
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Resonance
Resonance
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Resonance Structures
Resonance Structures
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Molecular Geometry
Molecular Geometry
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Hybridization
Hybridization
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Intermolecular Forces
Intermolecular Forces
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Metalloids
Metalloids
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Study Notes
The Periodic Table
- Fluorine has the highest electronegativity.
- Noble gases are located in Group 18 of the periodic table.
- Elements in the same group have the same number of valence electrons.
- Only metals are contained in Period 4.
- Silicon is an example of a metalloid.
- Magnesium is most likely to form a +2 ion.
- An element's placement in the periodic table is primarily determined by its atomic number.
Bonding
- Ionic bonds are typically formed between a metal and a nonmetal.
- Covalent bonds involve the sharing of electrons.
- NaCl contains ionic bonds.
- A metallic bond is characterized as a sea of delocalized electrons.
- Na2SO4 contains both ionic and covalent bonds.
- Electrons are shared unequally in a polar covalent bond.
- The correct Lewis structure for water (H2O) is H-O-H with two lone pairs on oxygen
- Hybridization explains the combination of atomic orbitals.
- A complete transfer of electrons involves an ionic bond.
Lewis Structures
- Carbon has 4 valence electrons.
- Oxygen follows the octet rule in a Lewis structure.
- Oxygen typically has 2 lone pairs in a Lewis structure.
- The formal charge on oxygen in the Lewis structure of ozone (O3) is -1.
- The Lewis structure of SO42- has 32 total valence electrons.
- Boron does not follow the octet rule.
- Another name for a molecular orbital diagram, is condensed
Resonance
- Resonance occurs when the same molecule can be represented by multiple structures.
- A resonance hybrid is a mixture of multiple resonance structures.
- NO3-exhibits resonance.
- The actual structure of a resonance hybrid is an average of all resonance structures.
Molecular Shape
- CH4 has a tetrahedral molecular geometry.
- A molecule with three bonded atoms and one lone pair around the central atom has a trigonal pyramidal shape.
- NH3 has a trigonal pyramidal shape.
- The bond angle in methane (CH4) is approximately 109.5°.
- The shape of a water molecule determines molecular shape, according to VSEPR theory.
- A molecule with four bonding pairs and no lone pairs around the central atom has a tetrahedral shape.
- A molecule with two lone pairs and two bonded atoms on the central atom will have a bent geometry.
Hybridization
- The hybridization of carbon in ethene (C2H4) is sp².
- The hybridization of the central atom in CO2 is sp.
- Methane exhibits sp³ hybridization.
- Ethyne contains sp hybridized carbon.
- The number of hybrid orbitals in sp² hybridization is 3.
- In acetylene (C2H2), carbon has sp hybridization.
- Carbon dioxide exhibits sp³ hybridization
Bond Length and Bond Strength
- A triple bond is the strongest.
- As bond length decreases, bond strength increases.
- A stronger bond generally has a shorter bond length.
- A carbon-carbon single bond (C-C) is the longest.
- Bond length contributes to a greater influence on the strength of covalent bonds.
- The bond length of a single bond is generally longer than a double bond.
Electronegativity and Bond Polarity
- O-H has the highest polarity.
- A molecule with an electronegativity difference of 0.5 is considered a polar covalent.
- Caesium has the lowest electronegativity.
- An arrow points toward the more electronegative atom in a dipole moment.
Polarity of Molecules
- A polar molecule must have an unequal charge distribution.
- CO2 is a nonpolar molecule.
- Ammonia is polar.
- A symmetrical shape is required for a nonpolar molecule.
Intermolecular Forces, Hybridization, and Applications
- London dispersion forces are present in all molecules.
- Carbon is least likely to participate in hydrogen bonding.
- Hydrogen Flouride exhibits the strongest hydrogen bonding.
- London dispersion forces occur between two nonpolar molecules.
- Water's strongest intermolecular force is Hydrogen Bonding.
Other molecular properties
- As bond order increases, bond length decreases.
- Ammonia is most likely to have a distorted tetrahedral shape.
- The lone pair causes ammonia to have reduced bond angle.
- Carbon Tetrafluoride (CF4) is an example of a polar molecule with nonpolar bonds.
- A distorted molecular shape is called a 'seesaw' shape, due to the uneven weight
- The strongest intermolecular force in diatomic Bromine, is London Dispersion Force
- Molecular symmetry does not contribute to molecular polarity
- Diatomic halogens have London dispersions force as their intermolecular force.
- A bond between idnetical nonmetals, will always be nonpolar covalent
- Sigma bonds have the hightest electron density between the two nuclei.
- To calculate the formal charge of an atom use. Valence electrons minus nonbonding and half of bonding electrons.
- The bond order of nitrogen in N2 is 3.
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Description
Explores the periodic table's structure, electronegativity trends, and group properties. Discusses ionic, covalent, and metallic bonds, including electron sharing and Lewis structures. Covers examples like NaCl and Na2SO4.
