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Questions and Answers
What is the expected electron configuration for Copper (Cu)?
What is the expected electron configuration for Copper (Cu)?
- [Ar] 4s13d10
- [Ar] 4s23d9 (correct)
- [Ar] 4s24d9
- [Ar] 4s23d8
What does Hund's Rule state?
What does Hund's Rule state?
- Electrons occupy orbitals in pairs before any orbital is singly occupied.
- Every orbital is singly occupied before any orbital gets doubly occupied. (correct)
- All orbitals of the same energy must have one electron before any can have two.
- Electrons fill the lowest available energy levels first.
Electromagnetic waves are classified only based on their energy levels.
Electromagnetic waves are classified only based on their energy levels.
False (B)
What happens to an electron when it absorbs light?
What happens to an electron when it absorbs light?
The distance between two successive peaks of a wave is known as its ______.
The distance between two successive peaks of a wave is known as its ______.
What is the electron configuration for sodium using the shorthand method?
What is the electron configuration for sodium using the shorthand method?
The shorthand electron configuration can be used for period 1 elements.
The shorthand electron configuration can be used for period 1 elements.
Elements in family 7A typically gain 1 electron to achieve stability.
Elements in family 7A typically gain 1 electron to achieve stability.
An element must attain _____ valence electrons to be stable per the octet rule.
An element must attain _____ valence electrons to be stable per the octet rule.
Which of the following elements follows the duplet rule instead of the octet rule?
Which of the following elements follows the duplet rule instead of the octet rule?
Match the family of elements with their valence electron count:
Match the family of elements with their valence electron count:
Match the following types of electromagnetic radiation with their characteristics:
Match the following types of electromagnetic radiation with their characteristics:
When an atom loses an electron, it gains a _____ charge.
When an atom loses an electron, it gains a _____ charge.
How many periods are there in the periodic table?
How many periods are there in the periodic table?
Family A consists only of transition metals.
Family A consists only of transition metals.
What is the maximum number of electrons that can occupy an 's' orbital?
What is the maximum number of electrons that can occupy an 's' orbital?
The ______ state occurs when all energy levels in an atom are full.
The ______ state occurs when all energy levels in an atom are full.
Match the following types of orbitals with their maximum electron capacity:
Match the following types of orbitals with their maximum electron capacity:
Which group is known as the Noble Gases?
Which group is known as the Noble Gases?
According to the Pauli exclusion principle, two electrons in the same orbital must have the same spin.
According to the Pauli exclusion principle, two electrons in the same orbital must have the same spin.
What principle states that electrons fill the lowest available energy subshells first?
What principle states that electrons fill the lowest available energy subshells first?
What is the electron configuration of Yttrium (39)?
What is the electron configuration of Yttrium (39)?
Yttrium belongs to Group 2B.
Yttrium belongs to Group 2B.
How many valence electrons does Yttrium have?
How many valence electrons does Yttrium have?
Yttrium is located in Period __.
Yttrium is located in Period __.
What is the number of d-orbital electrons in Yttrium?
What is the number of d-orbital electrons in Yttrium?
Match the following properties to their values for Yttrium:
Match the following properties to their values for Yttrium:
The energy level of Yttrium is determined by its group number.
The energy level of Yttrium is determined by its group number.
What is the rule to find the Group number for Yttrium?
What is the rule to find the Group number for Yttrium?
Which element has the largest atomic radius?
Which element has the largest atomic radius?
The ionic size increases from left to right across a period.
The ionic size increases from left to right across a period.
Define ionization energy.
Define ionization energy.
The distance from the nucleus of a neutral atom to the outermost shell is called the atomic __________.
The distance from the nucleus of a neutral atom to the outermost shell is called the atomic __________.
Match the following ions with their expected size relationship:
Match the following ions with their expected size relationship:
What happens to atomic radius as you move from top to bottom in a group?
What happens to atomic radius as you move from top to bottom in a group?
Anions are always larger than their corresponding neutral atoms.
Anions are always larger than their corresponding neutral atoms.
When an atom loses electrons, its ionic size __________.
When an atom loses electrons, its ionic size __________.
Which of the following statements is correct regarding nonmetals?
Which of the following statements is correct regarding nonmetals?
The atomic size increases from left to right across the periodic table.
The atomic size increases from left to right across the periodic table.
What is the charge of a nitride ion?
What is the charge of a nitride ion?
The formula for sulfate ion is ______.
The formula for sulfate ion is ______.
Match the following ions with their corresponding formulas:
Match the following ions with their corresponding formulas:
Which element has the highest electronegativity?
Which element has the highest electronegativity?
The ionization energy increases as you move down a group in the periodic table.
The ionization energy increases as you move down a group in the periodic table.
What type of compound is formed when a cation pairs with an anion?
What type of compound is formed when a cation pairs with an anion?
A binary ionic compound is composed of ______ elements.
A binary ionic compound is composed of ______ elements.
Which property of metals increases from top to bottom in the periodic table?
Which property of metals increases from top to bottom in the periodic table?
What is the possible range of values for the electron spin quantum number (ms)?
What is the possible range of values for the electron spin quantum number (ms)?
An electron with a spin quantum number of -½ is said to be spinning in a clockwise direction.
An electron with a spin quantum number of -½ is said to be spinning in a clockwise direction.
What does a positive value of the electron spin quantum number (ms) indicate about the electron's spin?
What does a positive value of the electron spin quantum number (ms) indicate about the electron's spin?
The periodic law states that the physical and chemical properties of an element tend to vary periodically in order of increasing _______.
The periodic law states that the physical and chemical properties of an element tend to vary periodically in order of increasing _______.
Match the following electron configurations with their corresponding electron spin states:
Match the following electron configurations with their corresponding electron spin states:
Which scientist is known as the Father of the Periodic Table?
Which scientist is known as the Father of the Periodic Table?
Henry Moseley arranged elements by their atomic mass.
Henry Moseley arranged elements by their atomic mass.
What did John Newlands contribute to the development of the periodic table?
What did John Newlands contribute to the development of the periodic table?
The average of the atomic masses of the first and third elements in Döbereiner's triads is equal to the atomic mass of the ______ element.
The average of the atomic masses of the first and third elements in Döbereiner's triads is equal to the atomic mass of the ______ element.
Match each scientist with their contribution to the periodic table:
Match each scientist with their contribution to the periodic table:
What major change did Moseley make to the arrangement of the periodic table?
What major change did Moseley make to the arrangement of the periodic table?
Döbereiner’s Law of Triads is based on the atomic number of elements.
Döbereiner’s Law of Triads is based on the atomic number of elements.
The periodic table is a tabular arrangement of chemical elements organized according to increasing ______.
The periodic table is a tabular arrangement of chemical elements organized according to increasing ______.
Which electron configuration corresponds to the element with 8 valence electrons in Group 8A and Period 2?
Which electron configuration corresponds to the element with 8 valence electrons in Group 8A and Period 2?
The maximum number of electrons that can occupy a p orbital is 8.
The maximum number of electrons that can occupy a p orbital is 8.
Identify the element that has the electron configuration 1s2 2s2 2p6.
Identify the element that has the electron configuration 1s2 2s2 2p6.
In period 2, family 8A, the total number of electrons is _____.
In period 2, family 8A, the total number of electrons is _____.
Match the following elements with their corresponding group and period:
Match the following elements with their corresponding group and period:
What happens to ionization energy as you move from left to right across a period?
What happens to ionization energy as you move from left to right across a period?
Electron affinity increases from top to bottom in a group.
Electron affinity increases from top to bottom in a group.
What is electronegativity?
What is electronegativity?
Ionization energy is opposite the atomic _____
Ionization energy is opposite the atomic _____
Match the following trends with their descriptions:
Match the following trends with their descriptions:
Which of the following statements about ionization energy is correct?
Which of the following statements about ionization energy is correct?
Higher electronegativity means an atom is more likely to lose electrons.
Higher electronegativity means an atom is more likely to lose electrons.
Explain why it is easier for atoms on the left side of the periodic table to lose electrons.
Explain why it is easier for atoms on the left side of the periodic table to lose electrons.
The Aufbau principle states that electrons fill the highest energy subshells first.
The Aufbau principle states that electrons fill the highest energy subshells first.
How many groups (families) are present in the periodic table?
How many groups (families) are present in the periodic table?
The group of elements known as ______ gases is found in family 8A.
The group of elements known as ______ gases is found in family 8A.
Match the following groups of elements with their corresponding names:
Match the following groups of elements with their corresponding names:
Which of the following best describes an excited state of an atom?
Which of the following best describes an excited state of an atom?
Which principle states that a maximum of two electrons may occupy an orbital if they have opposite spins?
Which principle states that a maximum of two electrons may occupy an orbital if they have opposite spins?
What is the primary factor that determines the charge of an element in family 1A?
What is the primary factor that determines the charge of an element in family 1A?
The valence electrons for noble gases like neon are considered when determining their stability.
The valence electrons for noble gases like neon are considered when determining their stability.
For an atom to be stable, it must follow the octet rule, which states that an element must attain _____ valence electrons.
For an atom to be stable, it must follow the octet rule, which states that an element must attain _____ valence electrons.
Match the elements to their corresponding group number based on valence electrons:
Match the elements to their corresponding group number based on valence electrons:
According to Hund’s Rule, how should electrons be filled in the orbitals?
According to Hund’s Rule, how should electrons be filled in the orbitals?
The electron configuration 1s22s22p6 is equivalent to the configuration of Argon.
The electron configuration 1s22s22p6 is equivalent to the configuration of Argon.
In family 6A, the charge of elements is typically _____ when they attain stability.
In family 6A, the charge of elements is typically _____ when they attain stability.
Flashcards
Periodic Table Periods
Periodic Table Periods
Horizontal rows in the periodic table; there are 7 periods.
Periodic Table Groups/Families
Periodic Table Groups/Families
Vertical columns in the periodic table, consisting of representative elements (A) and transition metals (B); total of 18.
Electron Configuration
Electron Configuration
Arrangement of electrons in atomic orbitals; the most stable state is the ground state.
Atomic Orbital
Atomic Orbital
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Ground State
Ground State
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Aufbau Principle
Aufbau Principle
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Pauli Exclusion Principle
Pauli Exclusion Principle
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Electron Spin
Electron Spin
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Electromagnetic Spectrum
Electromagnetic Spectrum
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Frequency (EM)
Frequency (EM)
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Wavelength (EM)
Wavelength (EM)
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Ground State (Electron)
Ground State (Electron)
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Excited State (Electron)
Excited State (Electron)
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Hund's Rule
Hund's Rule
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Shorthand electron configuration
Shorthand electron configuration
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Valence Electrons
Valence Electrons
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Octet Rule
Octet Rule
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Representative elements
Representative elements
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Valence electron family number
Valence electron family number
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Stable configuration
Stable configuration
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Electron Configuration Filling Order
Electron Configuration Filling Order
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Electron Configuration of Neon (Ne)
Electron Configuration of Neon (Ne)
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Group of Neon (Ne)
Group of Neon (Ne)
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Valence Electrons of Neon (Ne)
Valence Electrons of Neon (Ne)
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Period of Yttrium (Y)
Period of Yttrium (Y)
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Group Determination of Yttrium (Y)
Group Determination of Yttrium (Y)
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Valence Electrons of Yttrium (Y)
Valence Electrons of Yttrium (Y)
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Energy Level of Yttrium (Y)
Energy Level of Yttrium (Y)
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Electron Configuration for Yttrium (Y)
Electron Configuration for Yttrium (Y)
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Metallic Property
Metallic Property
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Nonmetallic Property
Nonmetallic Property
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Trend: Atomic Size in Periodic Table
Trend: Atomic Size in Periodic Table
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Trend: Ionization Energy in Periodic Table
Trend: Ionization Energy in Periodic Table
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Trend: Electron Affinity in Periodic Table
Trend: Electron Affinity in Periodic Table
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Trend: Electronegativity in Periodic Table
Trend: Electronegativity in Periodic Table
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Monatomic Ions
Monatomic Ions
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Polyatomic Ions
Polyatomic Ions
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Atomic Radius
Atomic Radius
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Atomic Radius Trend: Downward
Atomic Radius Trend: Downward
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Atomic Radius Trend: Rightward
Atomic Radius Trend: Rightward
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Ionic Radius
Ionic Radius
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Cation vs. Anion
Cation vs. Anion
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Ionic Radius Trend: Downward and Rightward
Ionic Radius Trend: Downward and Rightward
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Ionization Energy
Ionization Energy
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Ionization Energy Trend: Rightward
Ionization Energy Trend: Rightward
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Periodic Table
Periodic Table
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Döbereiner's Triads
Döbereiner's Triads
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Newlands' Law of Octaves
Newlands' Law of Octaves
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Mendeleev's Periodic Table
Mendeleev's Periodic Table
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Moseley's Periodic Table
Moseley's Periodic Table
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Period
Period
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Group
Group
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How to determine the electron configuration of an element using Group and Period
How to determine the electron configuration of an element using Group and Period
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What are periods in the periodic table?
What are periods in the periodic table?
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What are groups in the periodic table?
What are groups in the periodic table?
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What is the difference between groups A and B?
What is the difference between groups A and B?
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What are valence electrons?
What are valence electrons?
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What is electron configuration?
What is electron configuration?
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What is the Aufbau principle?
What is the Aufbau principle?
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What is the Pauli Exclusion Principle?
What is the Pauli Exclusion Principle?
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What is Hund's Rule?
What is Hund's Rule?
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Electron Spin Quantum Number (ms)
Electron Spin Quantum Number (ms)
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What does +1/2 ms value represent?
What does +1/2 ms value represent?
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Atomic Size Trend: Rightward
Atomic Size Trend: Rightward
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Ionization Energy Trend: Across a Period
Ionization Energy Trend: Across a Period
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Ionization Energy Trend: Down a Group
Ionization Energy Trend: Down a Group
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Electron Affinity Trend: Across a Period
Electron Affinity Trend: Across a Period
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Electron Affinity Trend: Down a Group
Electron Affinity Trend: Down a Group
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Electronegativity Trend: Across a Period
Electronegativity Trend: Across a Period
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Electronegativity Trend: Down a Group
Electronegativity Trend: Down a Group
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What is Electron Affinity?
What is Electron Affinity?
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What is Electronegativity?
What is Electronegativity?
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Study Notes
Chemistry Study Notes
- Q1 9-CONCHEM: This likely refers to a specific unit or chapter in a Chemistry course, within the first quarter
- Q2 9-CONCHEM: Similar to Q1, this likely refers to a chemistry unit or chapter in the second quarter of the semester
- UNIT IV: Order Among Elements: This unit covers the development and organization of the periodic table, including chemical symbols, electron configuration, group numbers, valence electrons, and trends in the periodic table
- UNIT V: Stoichiometry: This unit discusses calculations related to chemical reactions, including chemical formulas, mole concept, molar mass, percentage composition, empirical and molecular formulas, balancing chemical equations, types of chemical reactions, and calculations based on balanced equations
- UNIT VI: Chemical Bond: This section covers types of chemical bonds (ionic, covalent, metallic), octet rule, Lewis symbols, bond polarity, electronegativity, molecular geometry and intermolecular forces
- 4.1-3 The Periodic Table: This section of the notes explains how the periodic table is organized and arranged and includes the historical development of the periodic table
- 1817: Johann Wolfgang Döbereiner's Law of Triads: Döbereiner grouped elements into sets of three exhibiting similar properties. The average of the atomic mass of the first and third element approximates the second element's atomic weight
- 1865: John Newlands's Law of Octaves: Newlands arranged elements based on increasing atomic mass. Elements with similar properties recurred every eighth element (like an octave in music) (applicable to elements before Calcium).
- 1869: Dmitri Mendeleev's Periodic Table: Mendeleev's table organized by increasing atomic number. It contained spaces for undiscovered elements
- 1913: Henry Moseley's Periodic Table: This modern periodic table is organized by atomic number, not atomic mass, leading to a more accurate arrangement.
- 4.4 Electron Configuration: Explains the distribution of electrons in atomic orbitals, including ground and excited states, and the principles of Aufbau, Hund's rule, and Pauli exclusion to determine the electron configuration
- 4.5 Valence Electrons and Blocks: This explains valence electrons (electrons in the outermost shell), the octet rule, how to relate valence electrons to the group number, and how they are organized in blocks in the periodic table
- 4.6 Electromagnetic Radiation and Quantum Numbers: This section covers the structure and properties of electromagnetic waves, the full electromagnetic spectrum, and relationships among energy, wavelength, frequency to understand quantum behavior and properties
- 4.7 Periodic Trends: This unit addresses how atomic properties like atomic size, ionization energy, electron affinity, electronegativity, metallic, and non-metallic properties change across a period and down a group.
- UNIT V: Stoichiometry - Monatomic lons: Provides a table for monatomic ions and their charges (e.g. Li+, Na+, Mg2+, Al3+, etc.)
- UNIT V: Stoichiometry - Polyatomic Ions: Provides a table for polyatomic ions and their formulas (e.g. nitrate, sulfate, phosphate, hydroxide, carbonate, etc.)
- 5.1 Naming and Writing lonic Formulas: Explains the naming and writing of formulas for ionic compounds. Discusses the relationship between the charge of ions and the formulas of ionic compounds.
- 5.3 Balancing Chemical Equations: Explains chemical equations, how to balance chemical equations by adjusting coefficients to maintain the law of conservation of mass (the number of atoms of each element must be the same on both sides of the equation).
- Q3 9-CONCHEM, Q4 9-CONCHEM: These denote third and fourth quarter units or chapters in the 9-CONCHEM course, respectively.
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Description
Test your knowledge on vital concepts from Units IV to VI of Chemistry, including the Periodic Table, Stoichiometry, and Chemical Bonds. This quiz covers electron configurations, balancing equations, and molecular polarity. Prepare to demonstrate your understanding of the chemical behavior of elements and fundamental stoichiometric principles.
