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Questions and Answers
What does the Pauli exclusion principle state regarding electrons in an orbital?
What does the Pauli exclusion principle state regarding electrons in an orbital?
- Each orbital must contain at least one electron before any can be paired.
- Each orbital can contain any number of electrons regardless of their spin.
- Each orbital may contain no more than two electrons with the same spin.
- Each orbital can hold a maximum of two electrons with opposite spins. (correct)
According to Hund's rule, what is the preferred arrangement of electrons in p orbitals?
According to Hund's rule, what is the preferred arrangement of electrons in p orbitals?
- Electrons should fill the lower energy orbitals first regardless of the p sub-level.
- Electrons can only occupy orbitals based on their spin state.
- All electrons must pair up in the same orbital before occupying empty orbitals.
- Electrons should occupy half of the empty orbitals before pairing in the same orbital. (correct)
How many electrons can a single p sub-level hold at maximum?
How many electrons can a single p sub-level hold at maximum?
- 4 electrons in two orbitals including pairing.
- 8 electrons when considering all p orbitals.
- 6 electrons across three orbitals. (correct)
- 2 electrons in two separate orbitals.
What is the stability preference for electron arrangements in orbitals?
What is the stability preference for electron arrangements in orbitals?
Which type of orbital exists in the first shell?
Which type of orbital exists in the first shell?
Why does the 4s orbital contain one electron in larger atoms?
Why does the 4s orbital contain one electron in larger atoms?
How many p orbitals are present in the second shell?
How many p orbitals are present in the second shell?
Which of the following states the correct filling order of orbitals according to the Aufbau principle?
Which of the following states the correct filling order of orbitals according to the Aufbau principle?
What shape does an s orbital have?
What shape does an s orbital have?
What is the maximum number of electrons that an orbital can hold?
What is the maximum number of electrons that an orbital can hold?
Which of these rules states that each orbital must be filled singly before pairing?
Which of these rules states that each orbital must be filled singly before pairing?
Which of the following is true about the filling order of the third shell?
Which of the following is true about the filling order of the third shell?
What is the principal quantum number associated with the f orbitals?
What is the principal quantum number associated with the f orbitals?
What is the relative atomic mass of the sample of chlorine calculated in the content?
What is the relative atomic mass of the sample of chlorine calculated in the content?
What is the molar mass of sodium chloride (NaCl)?
What is the molar mass of sodium chloride (NaCl)?
How many moles are represented by 20 grams of a substance with a molar mass of 10 g/mol?
How many moles are represented by 20 grams of a substance with a molar mass of 10 g/mol?
Which of the following properties does NOT describe giant covalent substances?
Which of the following properties does NOT describe giant covalent substances?
What is the characteristic structure of diamond?
What is the characteristic structure of diamond?
Which carbon allotrope has good electrical conductivity due to delocalised electrons?
Which carbon allotrope has good electrical conductivity due to delocalised electrons?
How many particles are in one mole as described by Avogadro’s number?
How many particles are in one mole as described by Avogadro’s number?
Which of the following describes the bonding in giant covalent substances?
Which of the following describes the bonding in giant covalent substances?
What is the calculated number of moles in 2.842 g of sodium sulfate, Na2SO4?
What is the calculated number of moles in 2.842 g of sodium sulfate, Na2SO4?
How do you determine the empirical formula of a compound?
How do you determine the empirical formula of a compound?
What is the relative formula mass (RFM) of chlorine given 80% chlorine-35 and 20% chlorine-37?
What is the relative formula mass (RFM) of chlorine given 80% chlorine-35 and 20% chlorine-37?
Given 828 g of lead and 64 g of oxygen, which of the following represents the empirical formula?
Given 828 g of lead and 64 g of oxygen, which of the following represents the empirical formula?
What is the primary reason for the malleability and ductility of metals?
What is the primary reason for the malleability and ductility of metals?
For a compound with a relative formula mass of 32 consisting of 87.5% nitrogen and 12.5% hydrogen, what is the empirical formula?
For a compound with a relative formula mass of 32 consisting of 87.5% nitrogen and 12.5% hydrogen, what is the empirical formula?
Which of the following correctly describes covalent substances?
Which of the following correctly describes covalent substances?
Which statement about metallic bonding is true?
Which statement about metallic bonding is true?
Which step is NOT part of finding an empirical formula?
Which step is NOT part of finding an empirical formula?
How many moles are present in 6.02 g of magnesium sulfate, MgSO4?
How many moles are present in 6.02 g of magnesium sulfate, MgSO4?
What is the relative atomic mass (Ar) of an element calculated from?
What is the relative atomic mass (Ar) of an element calculated from?
Which property of metallic substances is primarily due to delocalised electrons?
Which property of metallic substances is primarily due to delocalised electrons?
What is the first step in calculating the empirical formula for a sample of elements?
What is the first step in calculating the empirical formula for a sample of elements?
Which combination of isotopic abundances is used to calculate the relative atomic mass of chlorine?
Which combination of isotopic abundances is used to calculate the relative atomic mass of chlorine?
How do simple covalent substances differ from metallic bonding in their electrical conductivity?
How do simple covalent substances differ from metallic bonding in their electrical conductivity?
What structural feature characterizes a giant metallic lattice?
What structural feature characterizes a giant metallic lattice?
What does a saturated solution imply?
What does a saturated solution imply?
Which statement accurately describes a solute?
Which statement accurately describes a solute?
What represents the Law of Conservation of Mass in a chemical reaction?
What represents the Law of Conservation of Mass in a chemical reaction?
What does the coefficient in a balanced chemical equation indicate?
What does the coefficient in a balanced chemical equation indicate?
How is molarity calculated?
How is molarity calculated?
What defines supersaturation in a solution?
What defines supersaturation in a solution?
Which of the following is a characteristic of a reactant in a chemical equation?
Which of the following is a characteristic of a reactant in a chemical equation?
In the empirical formula analysis, what does a subscript represent?
In the empirical formula analysis, what does a subscript represent?
Flashcards
Empirical Formula
Empirical Formula
The simplest whole number ratio of atoms or ions in a compound.
Relative Formula Mass (RFM)
Relative Formula Mass (RFM)
The mass of one mole of a substance. It's like the 'unit weight' of a compound.
Orbital Capacity
Orbital Capacity
Each orbital can hold a maximum of two electrons.
Group Electron Configuration
Group Electron Configuration
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Pauli Exclusion Principle
Pauli Exclusion Principle
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Hund's Rule
Hund's Rule
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Chromium and Copper Exceptions
Chromium and Copper Exceptions
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Metallic Bonding
Metallic Bonding
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Delocalized Electrons in Metallic Bonding
Delocalized Electrons in Metallic Bonding
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Giant Metallic Lattice
Giant Metallic Lattice
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High Melting and Boiling Points of Metals
High Melting and Boiling Points of Metals
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Good Electrical Conductivity of Metals
Good Electrical Conductivity of Metals
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Malleability and Ductility of Metals
Malleability and Ductility of Metals
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Relative Molecular Mass
Relative Molecular Mass
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Calculating Relative Atomic Mass
Calculating Relative Atomic Mass
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Solute
Solute
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Saturated Solution
Saturated Solution
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Supersaturation
Supersaturation
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Chemical Equation
Chemical Equation
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Reactants
Reactants
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Products
Products
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Subscript
Subscript
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Coefficient
Coefficient
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What are Atomic Orbitals?
What are Atomic Orbitals?
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What is an Electron Shell?
What is an Electron Shell?
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What are Electronic Configurations?
What are Electronic Configurations?
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What is the Aufbau Principle?
What is the Aufbau Principle?
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What are Types of Orbitals?
What are Types of Orbitals?
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What is the Filling Order of Electron Shells?
What is the Filling Order of Electron Shells?
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What is Hund's Rule?
What is Hund's Rule?
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What is Electron Configuration?
What is Electron Configuration?
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What is Avogadro's number?
What is Avogadro's number?
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What is a mole?
What is a mole?
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What is a giant covalent structure?
What is a giant covalent structure?
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What are the properties of giant covalent structures?
What are the properties of giant covalent structures?
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What are the properties of diamond?
What are the properties of diamond?
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What are the properties of graphite?
What are the properties of graphite?
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What is relative atomic mass?
What is relative atomic mass?
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How to calculate molar mass?
How to calculate molar mass?
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Study Notes
Atomic Structure
- Atoms are the smallest particles of chemical elements.
- Elements are substances with atoms having the same number of protons (atomic number).
- Protons are positively charged subatomic particles found in the atomic nucleus.
- Neutrons are neutral subatomic particles also found in the atomic nucleus.
- Electrons are negatively charged subatomic particles, much smaller than protons or neutrons.
- The nucleus is the positively charged central core of an atom, containing protons and neutrons.
- Almost all of an atom's mass is concentrated in its nucleus.
- Atomic number is the number of protons in an atom's nucleus.
- Isotopes are forms of the same element with the same number of protons but different numbers of neutrons, and therefore different masses.
- Mass number is the total number of protons and neutrons in an atom's nucleus.
- Relative atomic mass (Ar) is the ratio of the average mean mass of one atom of an element to one-twelfth the mass of an atom of carbon-12.
Periodic Table
- The order of elements in the periodic table is determined by their atomic number.
- An element's position in the periodic table is also determined by its electronic structure, especially the outermost electron shell.
- The number of electrons in the outermost shell determines the element's group.
- The number of electron shells determines the period an element is in.
Electronic Arrangement
- Shells (energy levels) are described by a principal quantum number (n).
- Each shell can hold up to 2n² electrons.
- Different shells have different quantum numbers.
- Electrons fill shells and sub-levels starting with the lowest energy levels first.
- Sub-levels are s, p, d, and f.
- Each sublevel holds a different maximum number of electrons (s = 2, p = 6, d = 10, f = 14).
- Orbitals are regions within an atom that contain electrons having opposite spins.
Electronic Configurations
- The Aufbau principle describes how electrons fill atomic orbitals.
- Electrons first fill the lowest energy levels.
- Any orbital can hold a maximum of two electrons with opposite spins.
Ionic Bonding
- Involves the transfer of electrons between metal and non-metal atoms.
- Metals lose electrons to form positive ions (cations).
- Non-metals gain electrons to form negative ions (anions).
- The electrostatic attraction between these oppositely charged ions forms the ionic bond.
- lons are arranged in a crystal lattice structure.
- lonic compounds are typically solid at room temperature and have high melting and boiling points.
Covalent Bonding
- Involves the sharing of electrons between non-metal atoms.
- A covalent bond consists of a shared pair of electrons.
- Covalent bonds are usually directional.
- Properties of covalent bonds include low melting and boiling points, where covalent substances may exist as a solid, liquid or gas at room temperature.
- Covalent compounds do not conduct electricity, as solids or liquids.
- Dative covalent (coordinate) bonds are a type of covalent bond where both electrons in the shared pair come from the same atom.
Metallic Bonding
- Involves a lattice of positive metal ions surrounded by a "sea" of delocalised electrons.
- Delocalised electrons are free to move throughout the lattice, giving rise to the electrical conductivity of metals.
- The strong electrostatic attraction between the ions and delocalised electrons gives metals high melting and boiling points.
- Metals are malleable and ductile, due to the layers of metal ions that can slide past one another.
Mole Calculations
- Relative molecular mass (Mr) is the sum of the atomic masses of all atoms in a molecule.
- Moles (n) = mass (g) / Mr (g/mol).
- Avogadro's constant is the number of atoms, molecules, or ions in one mole (6.02 x 10²³).
Empirical Formula
- The empirical formula is the simplest whole number ratio of atoms of each element in a compound.
Percent Yield
- Percentage Yield is a calculation that compares the amount of product made in a chemical reaction to the theoretical yield.
Limiting Reagent
- The limiting reagent is the reactant that determines the maximum amount of product that can be formed in a chemical reaction.
Intermolecular Forces
- London dispersion forces (temporary dipole-induced dipole forces) are weak intermolecular forces that act between all molecules, including nonpolar ones.
- Dipole-dipole forces are stronger than London dispersion forces and act only between polar molecules.
- Hydrogen bonds are a special type of dipole-dipole interaction that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine).
Polar and Non-Polar Molecules
- Polar molecules have a positive and negative end due to uneven electron distribution.
- Non-polar molecules have an even distribution of electrons, resulting in no separation of charge.
- Electronegativity is the tendency of an atom to attract bonding electrons to itself.
Balancing Chemical Equations
- Equations must follow the law of conservation of mass, stating that the number and type of atoms must remain the same on both sides of the equation.
- Coefficients are used to balance chemical equations, modifying the number of molecules to ensure the quantity of each element is equal on both sides.
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Description
Test your knowledge on the fundamental concepts of atomic structure, including the types of subatomic particles, atomic numbers, isotopes, and relative atomic mass. This quiz will help reinforce your understanding of how atoms are organized and their significance in the realm of chemistry.
