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Questions and Answers
Questions and Answers
The Lewis structure of N2H2 shows ________.
The Lewis structure of N2H2 shows ________.
each nitrogen has one nonbonding electron pair
The Lewis structure of AsH3 shows ________ nonbonding electron pair(s) on As.
The Lewis structure of AsH3 shows ________ nonbonding electron pair(s) on As.
1
The formal charge on nitrogen in NO3- is ________.
The formal charge on nitrogen in NO3- is ________.
+1
In the Lewis structure of HCO3-, the formal charge on H is ________, and the formal charge on C is ________.
In the Lewis structure of HCO3-, the formal charge on H is ________, and the formal charge on C is ________.
The definition of STP is
The definition of STP is
One mole of which gas will occupy 22.4 L at STP?
One mole of which gas will occupy 22.4 L at STP?
What is the volume occupied by 3.70 moles of N2 gas at STP?
What is the volume occupied by 3.70 moles of N2 gas at STP?
What is the value of the bond angles in CCl4?
What is the value of the bond angles in CCl4?
What is the value of the bond angle in XeCl2?
What is the value of the bond angle in XeCl2?
What is the value of the bond angles in COH2?
What is the value of the bond angles in COH2?
A sample of an ideal gas (3.00 L) in a closed container at 25.0 °C and 76.0 torr is heated to 290 °C. The pressure of the gas at this temperature is ________ torr.
A sample of an ideal gas (3.00 L) in a closed container at 25.0 °C and 76.0 torr is heated to 290 °C. The pressure of the gas at this temperature is ________ torr.
A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is ________ atm.
A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is ________ atm.
How many molecules are there in 4.00 L of oxygen gas at 500 °C and 50.0 torr?
How many molecules are there in 4.00 L of oxygen gas at 500 °C and 50.0 torr?
The temperature and pressure specified by STP are ________ °C and ________ atm.
The temperature and pressure specified by STP are ________ °C and ________ atm.
At a temperature of ________ °C, 0.444 mol of CO gas occupies 11.8 L at 923 torr.
At a temperature of ________ °C, 0.444 mol of CO gas occupies 11.8 L at 923 torr.
The molar volume of a gas at STP is ________ L.
The molar volume of a gas at STP is ________ L.
The mass of nitrogen dioxide contained in a 4.32 L vessel at 48 °C and 141600 Pa is ________ g.
The mass of nitrogen dioxide contained in a 4.32 L vessel at 48 °C and 141600 Pa is ________ g.
What is the density (in g/L) of oxygen gas at 77.0 °C and 700.0 torr?
What is the density (in g/L) of oxygen gas at 77.0 °C and 700.0 torr?
The density of HCl is ________ g/L at STP.
The density of HCl is ________ g/L at STP.
10.0 grams of argon and 20.0 grams of neon are placed in a 1070.0 ml container at 30.0 °C. The partial pressure of neon is ________ atm.
10.0 grams of argon and 20.0 grams of neon are placed in a 1070.0 ml container at 30.0 °C. The partial pressure of neon is ________ atm.
What is the partial pressure (in mm Hg) of neon in a 4.00 L vessel that contains 0.838 mol of methane, 0.184 mol of ethane, and 0.755 mol of neon at a total pressure of 928 mm Hg?
What is the partial pressure (in mm Hg) of neon in a 4.00 L vessel that contains 0.838 mol of methane, 0.184 mol of ethane, and 0.755 mol of neon at a total pressure of 928 mm Hg?
A vessel contained N2, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was ________ torr.
A vessel contained N2, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was ________ torr.
A sample of He gas (3.0 L) at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was ________ atm.
A sample of He gas (3.0 L) at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was ________ atm.
The principal quantum number of the electrons that are lost when yttrium forms a cation is ________.
The principal quantum number of the electrons that are lost when yttrium forms a cation is ________.
How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom?
How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom?
How many different types of resonance structures can be drawn for the ion SO32- where all atoms satisfy the octet rule?
How many different types of resonance structures can be drawn for the ion SO32- where all atoms satisfy the octet rule?
The hybrid orbitals used for bonding by the sulfur atom in the SF4 molecule are ________ orbitals.
The hybrid orbitals used for bonding by the sulfur atom in the SF4 molecule are ________ orbitals.
The hybridizations of nitrogen in NF3 and NH3 are ________ and ________, respectively.
The hybridizations of nitrogen in NF3 and NH3 are ________ and ________, respectively.
Of the molecules below, only ________ is nonpolar.
Of the molecules below, only ________ is nonpolar.
A nonpolar bond will form between two ____ atoms of ______ electronegativity.
A nonpolar bond will form between two ____ atoms of ______ electronegativity.
Of the following molecules, only ________ is polar.
Of the following molecules, only ________ is polar.
The molecular geometry of the NO2- molecule is ________, and this molecule is ________.
The molecular geometry of the NO2- molecule is ________, and this molecule is ________.
For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity?
For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity?
Of the molecules below, only ________ is polar.
Of the molecules below, only ________ is polar.
The molecular geometry of the PF3 molecule is ________, and this molecule is ________.
The molecular geometry of the PF3 molecule is ________, and this molecule is ________.
The electron-domain geometry and molecular geometry of the nitrite ion are ________ and ________, respectively.
The electron-domain geometry and molecular geometry of the nitrite ion are ________ and ________, respectively.
The central Xe atom in the XeF4 molecule has ________ unbonded electron pair(s) and ________ bonded electron pair(s) in its valence shell.
The central Xe atom in the XeF4 molecule has ________ unbonded electron pair(s) and ________ bonded electron pair(s) in its valence shell.
The molecular geometry of the PF4+ ion is ________.
The molecular geometry of the PF4+ ion is ________.
The molecular geometry of the SiH2Cl2 molecule is ________.
The molecular geometry of the SiH2Cl2 molecule is ________.
Linear bond angle is ________ degrees.
Linear bond angle is ________ degrees.
Linear Hybridization is ________.
Linear Hybridization is ________.
Trigonal Planar Angle is ________ degrees.
Trigonal Planar Angle is ________ degrees.
Trigonal Planar Hybridization is ________.
Trigonal Planar Hybridization is ________.
Tetrahedral bond angle is ________ degrees.
Tetrahedral bond angle is ________ degrees.
Tetrahedral Hybridization is ________.
Tetrahedral Hybridization is ________.
Triangular Bipyramidal bond angle is ________ degrees.
Triangular Bipyramidal bond angle is ________ degrees.
Triangular Bipyramidal Hybridization is ________.
Triangular Bipyramidal Hybridization is ________.
Octahedral bond angle is ________ degrees.
Octahedral bond angle is ________ degrees.
Octahedral Hybridization is ________.
Octahedral Hybridization is ________.
Linear (X-A-X) is ________.
Linear (X-A-X) is ________.
Linear (X-A-Y) is ________.
Linear (X-A-Y) is ________.
A BENT molecule looks like this: / \ X X is ________.
A BENT molecule looks like this: / \ X X is ________.
Trigonal Planar X / \ X X is ________.
Trigonal Planar X / \ X X is ________.
Trigonal Planar X / \ X Y is ________.
Trigonal Planar X / \ X Y is ________.
Tetrahedral X | X -- A / \ X X is ________.
Tetrahedral X | X -- A / \ X X is ________.
Tetrahedral X | X -- A / \ X Y is ________.
Tetrahedral X | X -- A / \ X Y is ________.
Polarity ________ as you go right across the periodic table.
Polarity ________ as you go right across the periodic table.
Which of the following has the bonds correctly arranged in order of increasing polarity?
Which of the following has the bonds correctly arranged in order of increasing polarity?
Questions and Answers
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Study Notes
Study Notes
Lewis Structures and Formal Charges
- The Lewis structure of N2H2 indicates that each nitrogen has one nonbonding electron pair.
- AsH3 has one nonbonding electron pair on arsenic (As).
- In NO3-, the formal charge on nitrogen is +1.
- For HCO3-, both hydrogen and carbon have a formal charge of 0.
Standard Temperature and Pressure (STP)
- Standard Temperature and Pressure (STP) is defined as 273 K and 1 atm.
- At STP, one mole of any gas occupies a volume of 22.4 L.
Gas Laws and Calculations
- To calculate the volume occupied by N2 gas at STP for 3.70 moles, apply the ideal gas law yielding 84.0 L.
- The decomposition of calcium carbonate produces carbon dioxide and calcium oxide.
- Using the ideal gas law, calculate the final pressure of a gas heated from 25.0 °C to 290 °C as 144 torr.
- Expand a gas (5.0 mol) at constant temperature from 10 L to 15 L results in a final pressure of 0.67 atm.
- Boyle's Law indicates the pressure when volume reduces using the formula P1V1 = P2V2, resulting in 924 torr when volume reduces to 8.13 L.
Bond Angles and Molecular Geometry
- The bond angle in CCl4 is measured at 109.5 degrees, indicating tetrahedral geometry.
- XeCl4 has a smallest bond angle of 90 degrees.
- COH2 has a bond angle of 120 degrees.
- XeCl2 exhibits a bond angle of 180 degrees.
- The molecular geometry of NO2- is bent and polar.
- PF3 has a trigonal pyramidal geometry and is polar.
- In PF4+, the geometry is tetrahedral.
Molecular Polarity and Resonance
- Molecules with no lone pairs, such as BF3, are nonpolar; however, others with lone pairs (e.g., AsH3) are polar.
- A nonpolar bond occurs between two identical atoms with equal electronegativity.
- For SO3, three equivalent resonance structures can be drawn without violating the octet rule.
- The ion SO32- has only one resonance structure that satisfies the octet rule.
Hybridization
- Nitrogen in NF3 and NH3 exhibits sp^3 hybridization.
- Sulfur in SF4 uses sp^3d hybridization for bonding.
- The central atom Xe in XeF4 has 2 lone and 4 bonded electron pairs in its valence shell.
Gas Density and Partial Pressure
- The density of oxygen gas at given conditions (77.0 °C and 700.0 torr) is calculated as 1.03 g/L.
- The partial pressure of neon in a vessel with various gases can be determined by Dalton's Law.
Quantum Number and Ideal Gas Concepts
- Yttrium loses electrons with a principal quantum number of 5 when forming a cation.
- The total pressure in mixtures can be calculated by combining the partial pressures and using appropriate gas laws.
General Concepts
- Polarity increases across the periodic table from left to right.
- The arrangement of bonds in order of increasing polarity indicates that the correct sequence is O—F, N—F, Be—F, Mg—F.
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