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Questions and Answers
What is the purpose of an empirical formula?
What is the purpose of an empirical formula?
- To depict how atoms are bonded in a compound
- To determine the molecular mass of a compound
- To show the elements present in a compound (correct)
- To calculate the number of atoms in a molecule
Which type of bond information is NOT provided by a structural formula?
Which type of bond information is NOT provided by a structural formula?
- Ionic bond (correct)
- Double covalent bond
- Single covalent bond
- Triple covalent bond
How is the formula mass different from the molecular mass?
How is the formula mass different from the molecular mass?
- Formula mass shows the exact number of atoms, while molecular mass doesn't
- Formula mass includes all types of bonds, while molecular mass only includes covalent bonds
- Formula mass is the mass of one formula unit, while molecular mass is the mass of one molecule (correct)
- Formula mass is for ionic compounds, while molecular mass is for covalent compounds
Which formula would be most helpful in determining the number of atoms in a molecule?
Which formula would be most helpful in determining the number of atoms in a molecule?
If a compound has the empirical formula CH2O, what could be its molecular formula?
If a compound has the empirical formula CH2O, what could be its molecular formula?
What is the empirical formula of the compound that contains 40.9% C, 4.58% H, and 54.51% O by mass?
What is the empirical formula of the compound that contains 40.9% C, 4.58% H, and 54.51% O by mass?
In the compound with 30.43% N and 69.57% O by mass, what is the molecular formula?
In the compound with 30.43% N and 69.57% O by mass, what is the molecular formula?
If a compound has a molecular weight of 180 g/mol and contains 40.0% C, 6.6% H, and 53.4% O, what is its molecular formula?
If a compound has a molecular weight of 180 g/mol and contains 40.0% C, 6.6% H, and 53.4% O, what is its molecular formula?
What is the empirical formula for a compound that consists of 49.5% C, 5.20% H, 28.8% N, and 16.5% O by mass?
What is the empirical formula for a compound that consists of 49.5% C, 5.20% H, 28.8% N, and 16.5% O by mass?
Determine the molecular formula for a compound with a molecular weight of 194.1 g/mol and an empirical formula of CH2O.
Determine the molecular formula for a compound with a molecular weight of 194.1 g/mol and an empirical formula of CH2O.
A compound comprises 92 g/mol with 30.43% N and 69.57% O by mass. What is its empirical formula?
A compound comprises 92 g/mol with 30.43% N and 69.57% O by mass. What is its empirical formula?
What is the empirical formula defined as?
What is the empirical formula defined as?
How does the percent composition of a compound relate to its empirical formula?
How does the percent composition of a compound relate to its empirical formula?
In the compound containing 25.93% nitrogen and 74.07% oxygen, what is the empirical formula?
In the compound containing 25.93% nitrogen and 74.07% oxygen, what is the empirical formula?
What does stoichiometry deal with in chemistry?
What does stoichiometry deal with in chemistry?
What information does the molecular formula provide about a compound?
What information does the molecular formula provide about a compound?
How are subscripts represented in an empirical formula?
How are subscripts represented in an empirical formula?
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Study Notes
Stoichiometry
- Branch of chemistry that deals with quantitative laws of chemical combination
- Concerned with measurements based on chemical combination
Empirical Formula
- Simplest formula for a compound, defined as the ratio of subscripts of the smallest possible whole number of elements present
- Also known as the simplest formula
- Gives information about the ratio of numbers of atoms in a compound
- Can be determined from percent composition of a compound
Examples of Empirical Formula
- PtCl2N2H6 (Cisplatin) from 65.0% Pt, 23.6% Cl, 9.35% N, and 2.05% H by mass
- NO3 from 25.93% N and 74.07% O
- C4H5N2O from 49.5% C, 5.20% H, 28.8% N, and 16.5% O by mass
- CH2O from 40.0% C, 6.6% H, and 53.4% O by mass
- NO2 from 30.43% N and 69.57% O
Molecular Formula
- Formula that shows the actual number of atoms of each element in a compound
- Can be determined from empirical formula and molecular mass
- Examples: C6H12O6 (Glucose), N2O4 (Dinitrogen tetroxide), C6H8O6 (Ascorbic acid or Vitamin C)
Structural Formula
- Displays the atoms of the molecule in the order they are bonded
- Shows how the atoms are bonded to one another (single, double, and triple covalent bonds)
- Examples: C3H8 (Propane), C4H10 (Butane), CH4 (Methane), C2H6 (Ethane)
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