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Questions and Answers
If an atom has an atomic number of 16, and a mass number of 32, what is the number of neutrons in its nucleus?
If an atom has an atomic number of 16, and a mass number of 32, what is the number of neutrons in its nucleus?
- 16 (correct)
- 32
- 48
- 8
An ion has a charge of +2. Which of the following statements is correct regarding the number of protons and electrons it contains?
An ion has a charge of +2. Which of the following statements is correct regarding the number of protons and electrons it contains?
- It has two more protons than electrons. (correct)
- It has two more electrons than protons.
- It has an equal number of protons and electrons.
- It has two more protons than neutrons.
Which subatomic particle primarily determines the identity of an element?
Which subatomic particle primarily determines the identity of an element?
- Positron
- Proton (correct)
- Electron
- Neutron
How does the number of electrons relate to the number of protons in a neutral atom?
How does the number of electrons relate to the number of protons in a neutral atom?
If an atom loses an electron, what type of ion does it form?
If an atom loses an electron, what type of ion does it form?
Which of the following statements accurately describes the relative masses of subatomic particles?
Which of the following statements accurately describes the relative masses of subatomic particles?
What is the mass number of an atom that contains 17 protons, 18 neutrons, and 17 electrons?
What is the mass number of an atom that contains 17 protons, 18 neutrons, and 17 electrons?
Which of the following describes the location of electrons within an atom?
Which of the following describes the location of electrons within an atom?
How does the concept of isotopes explain why the atomic weight listed on the periodic table is a decimal number?
How does the concept of isotopes explain why the atomic weight listed on the periodic table is a decimal number?
Which of these subatomic particle arrangements would result in a cation with a +2 charge?
Which of these subatomic particle arrangements would result in a cation with a +2 charge?
Which of the following electron configurations violates Hund's rule?
Which of the following electron configurations violates Hund's rule?
Consider an element with an atomic number of 8. How many electrons would be present in the corresponding ion with a -2 charge?
Consider an element with an atomic number of 8. How many electrons would be present in the corresponding ion with a -2 charge?
An element has the electron configuration $[Ar] 4s^2 3d^6$. In which block of the periodic table does it belong?
An element has the electron configuration $[Ar] 4s^2 3d^6$. In which block of the periodic table does it belong?
Which of the following elements has 6 valence electrons?
Which of the following elements has 6 valence electrons?
What change occurs at the electron level when an atom emits light, such as in the aurora borealis?
What change occurs at the electron level when an atom emits light, such as in the aurora borealis?
How does the quantum mechanical model describe the location of electrons in an atom?
How does the quantum mechanical model describe the location of electrons in an atom?
What is the valence shell of an element with the electronic configuration $1s^2 2s^2 2p^6 3s^2 3p^4$?
What is the valence shell of an element with the electronic configuration $1s^2 2s^2 2p^6 3s^2 3p^4$?
How many valence electrons does Strontium (Sr) have?
How many valence electrons does Strontium (Sr) have?
If an atom of an element has a mass number of 37 and contains 17 protons, how many neutrons does it have?
If an atom of an element has a mass number of 37 and contains 17 protons, how many neutrons does it have?
An element has the valence electron configuration of $ns^2 np^3$. Which group does it belong to in the periodic table?
An element has the valence electron configuration of $ns^2 np^3$. Which group does it belong to in the periodic table?
Element X has two isotopes: X-20 and X-22. If the atomic weight of element X is 20.8, which isotope is more abundant in nature?
Element X has two isotopes: X-20 and X-22. If the atomic weight of element X is 20.8, which isotope is more abundant in nature?
Which statement accurately describes the relationship between atomic number, mass number, and the number of electrons in a neutral atom?
Which statement accurately describes the relationship between atomic number, mass number, and the number of electrons in a neutral atom?
Which element is most likely to have similar chemical properties to Sulfur (S)?
Which element is most likely to have similar chemical properties to Sulfur (S)?
An element is located in the 5th period of the periodic table. According to the energy levels/shells principle, how many energy levels are occupied by its electrons?
An element is located in the 5th period of the periodic table. According to the energy levels/shells principle, how many energy levels are occupied by its electrons?
Tin (Sn) has the electron configuration ending in $5s^2 5p^2$. In which period and block of the periodic table is it located?
Tin (Sn) has the electron configuration ending in $5s^2 5p^2$. In which period and block of the periodic table is it located?
Which of the following statements accurately describes the relationship between energy levels and sublevels within an atom?
Which of the following statements accurately describes the relationship between energy levels and sublevels within an atom?
Consider an atom with electrons in the d sublevel. What is the maximum number of electrons that can occupy this sublevel?
Consider an atom with electrons in the d sublevel. What is the maximum number of electrons that can occupy this sublevel?
What does the Aufbau principle state regarding the filling of electron orbitals?
What does the Aufbau principle state regarding the filling of electron orbitals?
According to the Pauli Exclusion Principle, what is the maximum number of electrons that can occupy a single atomic orbital, and what must be true of their spins?
According to the Pauli Exclusion Principle, what is the maximum number of electrons that can occupy a single atomic orbital, and what must be true of their spins?
How does Hund's Rule of Maximum Multiplicity influence the arrangement of electrons within a sublevel containing multiple orbitals of equal energy (degenerate orbitals)?
How does Hund's Rule of Maximum Multiplicity influence the arrangement of electrons within a sublevel containing multiple orbitals of equal energy (degenerate orbitals)?
Which principle explains why electrons in the same orbital must have opposite spins?
Which principle explains why electrons in the same orbital must have opposite spins?
Consider the element Oxygen (O), which has 8 electrons. Based on the provided principles, how would its electrons be arranged in the 2p orbitals?
Consider the element Oxygen (O), which has 8 electrons. Based on the provided principles, how would its electrons be arranged in the 2p orbitals?
Which of the following elements has a valence shell with 6 electrons?
Which of the following elements has a valence shell with 6 electrons?
Which element's electron configuration ends with the last electron occupying a d orbital?
Which element's electron configuration ends with the last electron occupying a d orbital?
Which of the following represents the correct abbreviated electron configuration for Strontium (Sr)?
Which of the following represents the correct abbreviated electron configuration for Strontium (Sr)?
Which noble gas would be used to abbreviate the electron configuration of an element in the 4th period?
Which noble gas would be used to abbreviate the electron configuration of an element in the 4th period?
Considering the filling order of orbitals, which of the following subshells would be filled immediately after the 4_p_ subshell?
Considering the filling order of orbitals, which of the following subshells would be filled immediately after the 4_p_ subshell?
Which element is expected to have the same number of valence electrons as Gallium (Ga)?
Which element is expected to have the same number of valence electrons as Gallium (Ga)?
Which of the following statements accurately describes the noble gas configuration?
Which of the following statements accurately describes the noble gas configuration?
An element has an abbreviated electron configuration of [Kr] 5s² 4d². In which period of the periodic table is this element located?
An element has an abbreviated electron configuration of [Kr] 5s² 4d². In which period of the periodic table is this element located?
An element in Group 5A of the periodic table gains electrons to achieve a stable octet. What ionic charge will it typically have?
An element in Group 5A of the periodic table gains electrons to achieve a stable octet. What ionic charge will it typically have?
Chlorine (Cl) gains one electron to form a chloride ion (Cl-). Which statement accurately describes the change in its electronic configuration?
Chlorine (Cl) gains one electron to form a chloride ion (Cl-). Which statement accurately describes the change in its electronic configuration?
Sulfur (S) is in Group 6A. Which of the following options correctly identifies the number of valence electrons and the ionic charge of its ion?
Sulfur (S) is in Group 6A. Which of the following options correctly identifies the number of valence electrons and the ionic charge of its ion?
Consider an element 'X' that forms a stable ion with a 2+ charge. Which group in the periodic table is element 'X' MOST likely to belong to?
Consider an element 'X' that forms a stable ion with a 2+ charge. Which group in the periodic table is element 'X' MOST likely to belong to?
An unknown element 'Z' has an electronic configuration of 1s²2s²2p³. What ionic charge would 'Z' most likely adopt to achieve a noble gas configuration?
An unknown element 'Z' has an electronic configuration of 1s²2s²2p³. What ionic charge would 'Z' most likely adopt to achieve a noble gas configuration?
How does the number of protons and electrons change when a neutral atom of oxygen (O) forms an oxide ion (O²⁻)?
How does the number of protons and electrons change when a neutral atom of oxygen (O) forms an oxide ion (O²⁻)?
Which of the following electron configurations represents a stable ion MOST likely formed by an element in Group 6A?
Which of the following electron configurations represents a stable ion MOST likely formed by an element in Group 6A?
Which statement correctly describes the relationship between the group number of a representative nonmetal and its ionic charge?
Which statement correctly describes the relationship between the group number of a representative nonmetal and its ionic charge?
Flashcards
Atom
Atom
The smallest part of an element, retains properties.
Subatomic particles
Subatomic particles
Protons, neutrons, and electrons that make up an atom.
Proton
Proton
A positively charged particle located in the nucleus.
Neutron
Neutron
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Electron
Electron
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Atomic number (Z)
Atomic number (Z)
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Mass number (A)
Mass number (A)
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Neutral atom
Neutral atom
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X
X
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A
A
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Z
Z
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Isotopes
Isotopes
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Ion
Ion
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Cation
Cation
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Anion
Anion
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Quantum Mechanical Model
Quantum Mechanical Model
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Energy levels
Energy levels
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Quantum number (n)
Quantum number (n)
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Energy sublevels
Energy sublevels
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Maximum electron capacity per sublevel
Maximum electron capacity per sublevel
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Electron configuration
Electron configuration
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Aufbau's principle
Aufbau's principle
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Pauli's exclusion principle
Pauli's exclusion principle
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Hund's Rule of Maximum Multiplicity
Hund's Rule of Maximum Multiplicity
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Valence Shell
Valence Shell
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Valence Electrons
Valence Electrons
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Noble Gas Configurations
Noble Gas Configurations
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Abbreviated Configurations
Abbreviated Configurations
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Kernel Electron Configuration
Kernel Electron Configuration
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Energy/Orbital Diagrams
Energy/Orbital Diagrams
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Orbitals
Orbitals
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Periodic Table Groups
Periodic Table Groups
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Tin Electronic Configuration
Tin Electronic Configuration
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Period in Periodic Table
Period in Periodic Table
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Four Blocks of Elements
Four Blocks of Elements
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Representative Elements
Representative Elements
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Valence electrons in Group 7A
Valence electrons in Group 7A
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Chlorine's ionic charge
Chlorine's ionic charge
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Octet rule
Octet rule
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Ionic charge of sulfur
Ionic charge of sulfur
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Electron configuration of sulfur ion
Electron configuration of sulfur ion
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Group 6A nonmetals' valence electrons
Group 6A nonmetals' valence electrons
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Ionic charge of chlorine
Ionic charge of chlorine
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Ionic charge pattern by group
Ionic charge pattern by group
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Study Notes
Atomic Structure and Properties of Chemical Elements
- Atoms are the smallest parts of an element, retaining its properties.
- Atoms are composed of subatomic particles: protons, neutrons, and electrons.
- Protons are positively charged, located in the nucleus and have a mass of 1 amu.
- Neutrons have no charge, located in the nucleus, and have a mass of 1 amu.
- Electrons are negatively charged, located outside the nucleus, and have negligible mass (approximately 1/1836 amu).
- The atomic number (Z) is equal to the number of protons in an atom.
- The mass number (A) is the sum of protons and neutrons in an atom.
History of Atomic Models
- Solid Sphere Model (Dalton, 1803): Atoms are indivisible and identical for a given element.
- Plum Pudding Model (Thomson, 1904): Atoms contain negatively charged electrons embedded in a positively charged sphere.
- Nuclear Model (Rutherford, 1911): The atom is mostly empty space with a dense, positively charged nucleus at the center.
- Planetary Model (Bohr, 1913): Electrons orbit the nucleus in specific energy levels (orbits) that are quantized.
- Quantum Mechanical Model (Schrödinger, 1926): Electrons don't orbit in fixed paths but exist in probability clouds (orbitals) within energy levels.
Atomic Number, Mass Number, and Isotopes
- The atomic number defines the element.
- The mass number represents the total number of protons plus neutrons.
- Atoms of the same element with different numbers of neutrons are isotopes.
- Different isotopes have the same atomic number but different mass numbers.
- The average atomic mass of an element is determined by the relative abundance of its different isotopes.
Atomic Structure and Ions
- An ion is an atom or molecule that has a net electric charge due to a loss or gain of electrons.
- A positively charged ion is called a cation.
- A negatively charged ion is called an anion.
- Representative elements tend to form ions based on the number of electrons in their outermost shell (valence shell).
Electronic Configuration
- Electronic configuration describes the arrangement of electrons in different energy levels and sublevels within an atom.
- Aufbau's principle states that electrons fill the lowest energy orbitals first.
- Hund's rule states that electrons fill orbitals individually before pairing up.
- Pauli's exclusion principle states that only two electrons can occupy any given orbital, and they must have opposite spins.
- The periodic table organizes elements based on their electronic configurations.
- Valence electrons are electrons in the outermost shell of an atom. The number of valence electrons is often related to the group number on the periodic table.
Energy Levels and Sublevels
- Energy levels are designated by the principal quantum number (n).
- Sublevels within each energy level are designated by letters (s, p, d, f).
- Each sublevel has a specific number of orbitals, which specify the shape and spatial orientation of the electron cloud.
Orbital Diagrams
- Orbital diagrams are used to visualize the electronic distribution within each orbital.
- Pauli exclusion principle and Hund's rule guide the electron arrangement. Filling orbitals in order of energy and the direction of spin for each electron.
Noble Gas Configurations
- Noble gases have completely filled outermost electron shells. Their electron configuration is used to represent the configurations of other elements in an abbreviated form.
- The electronic configuration of a given element is abbreviated by preceding the noble gas symbol for the closest preceding element with a square bracket to express the electron configuration.
Types of Chemical Bonds
- Ionic Bonds: Transfer of electrons from a metal to a nonmetal, forming ions (cations and anions). The attractive forces between oppositely charged ions are a form of ionic bonding.
- Covalent Bonds: Sharing of valence electrons between two nonmetals or a nonmetal and a metalloid. This type of bonding does not result in ions.
Polar and Nonpolar Covalent Bonds
- Polar Covalent Bonds: The unequal sharing of electrons between atoms because the electronegativity between the two atoms differs.
- One atom has a greater attraction for the shared electrons, creating a partial positive charge on the one atom with the lesser attraction, and partial negative charge on the other atom receiving the electrons.
- Nonpolar Covalent Bonds: Equal sharing of electrons because the two elements sharing the electrons have similar electronegativities, so they have similar attractions.
Periodic Properties
- Elements in the same period show trends in properties (e.g., atomic radius, ionic radius, ionization energy, electronegativity.
- Metallic character generally increases from right to left across a period and from top to bottom within a group.
- Atomic radius generally increases from right to left across a period and from top to bottom within a group.
- Ionization energy and electronegativity generally increase from left to right across a period and from bottom to top within a group.
- Reactivity related to valence electrons often shows cyclical changes across the periodic table.
Octet Rule
- Atoms tend to gain, lose, or share electrons to achieve a stable electron configuration similar to a noble gas (8 valence electrons, except He).
The Structure of a Periodic Table
- Periods (horizontal rows) are numbered with integers (1 to 7) and indicate the number of electron shells.
- Group (vertical columns) are labeled with numbers from 1 to 18, sometimes including a letter (A or B). This indicates the number of valence electrons an element is expected to have.
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Test your knowledge of atomic structure. This includes understanding atomic number, mass number, ions, isotopes, and subatomic particles. Learn about protons, neutrons, and electrons.
