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Questions and Answers
Which of the following correctly lists the sublevels with their maximum number of electrons?
Which of the following correctly lists the sublevels with their maximum number of electrons?
- s2, p6, d10, f14 (correct)
- s2, p4, d6, f8
- s1, p2, d3, f4
- s1, p3, d5, f7
What is the number of orbitals found within the d sublevel?
What is the number of orbitals found within the d sublevel?
- 5 (correct)
- 3
- 1
- 7
According to quantum mechanics, how many electrons can occupy a single orbital within any sublevel?
According to quantum mechanics, how many electrons can occupy a single orbital within any sublevel?
- Depends on the sublevel.
- Two, if they have the same spin.
- Two, if they have opposite spins. (correct)
- One.
How many total electrons are required to completely fill the fourth energy level?
How many total electrons are required to completely fill the fourth energy level?
Which of the following orbital designations is not allowed according to the principles of quantum mechanics?
Which of the following orbital designations is not allowed according to the principles of quantum mechanics?
An atom has the following incorrect orbital notation:
- $1s^2: ↑↓$
- $2s^2: ↑↓$
- $2p^6: ↑↓ ↑↓ ↑↓$
- $3s^2: ↑↓$
- $3p^4: ↑↓ ↑ ↑$
Which rule or principle of electron configuration is broken in the $3p^4$ configuration, and why?
An atom has the following incorrect orbital notation:
- $1s^2: ↑↓$
- $2s^2: ↑↓$
- $2p^6: ↑↓ ↑↓ ↑↓$
- $3s^2: ↑↓$
- $3p^4: ↑↓ ↑ ↑$
Which rule or principle of electron configuration is broken in the $3p^4$ configuration, and why?
Which principle dictates that electrons first occupy the lowest energy levels available in an atom before filling higher energy levels?
Which principle dictates that electrons first occupy the lowest energy levels available in an atom before filling higher energy levels?
Which sublevel is characterized by a spherical electron cloud?
Which sublevel is characterized by a spherical electron cloud?
Which rule or principle is violated in the provided orbital notation for Diagram 3?
Which rule or principle is violated in the provided orbital notation for Diagram 3?
An element has the following abbreviated orbital notation: [Ne] 3s² 3p³. Which element is it?
An element has the following abbreviated orbital notation: [Ne] 3s² 3p³. Which element is it?
Which of the following orbital notations correctly represents Argon (Ar)?
Which of the following orbital notations correctly represents Argon (Ar)?
Which of the following electron configurations corresponds to an element in the third period (row) of the periodic table with 6 valence electrons?
Which of the following electron configurations corresponds to an element in the third period (row) of the periodic table with 6 valence electrons?
How many valence electrons does Cobalt (Co) possess, according to the provided information?
How many valence electrons does Cobalt (Co) possess, according to the provided information?
An element has the electron configuration $1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^{10}5p^66s^2$. Which element is it?
An element has the electron configuration $1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^{10}5p^66s^2$. Which element is it?
What is the expected number of electrons in the outermost shell (valence electrons) for Krypton (Kr)?
What is the expected number of electrons in the outermost shell (valence electrons) for Krypton (Kr)?
Given the incomplete electron configuration $1s^22s^22p^63s^23p^64s^23d^1$, which element does it represent?
Given the incomplete electron configuration $1s^22s^22p^63s^23p^64s^23d^1$, which element does it represent?
Elements located within the same group on the periodic table exhibit similarities in which characteristics?
Elements located within the same group on the periodic table exhibit similarities in which characteristics?
What feature do elements within the same period of the periodic table share?
What feature do elements within the same period of the periodic table share?
A period in the periodic table in which only the s and p sublevels are being filled contains how many elements?
A period in the periodic table in which only the s and p sublevels are being filled contains how many elements?
Which set of sublevels are being filled in a period that contains 32 elements?
Which set of sublevels are being filled in a period that contains 32 elements?
How can you determine the number of valence electrons in elements belonging to groups 13 through 18?
How can you determine the number of valence electrons in elements belonging to groups 13 through 18?
Which of the following elements is located in period 5, group 14 of the periodic table?
Which of the following elements is located in period 5, group 14 of the periodic table?
Which properties are characteristic of metals?
Which properties are characteristic of metals?
Which group contains the most reactive nonmetals, often used in disinfectants and water treatment?
Which group contains the most reactive nonmetals, often used in disinfectants and water treatment?
An element has the electron configuration $1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^2$. Which element does this represent?
An element has the electron configuration $1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^2$. Which element does this represent?
Which of the following noble gas configurations corresponds to antimony (Sb)?
Which of the following noble gas configurations corresponds to antimony (Sb)?
What is the noble gas configuration for technetium (Tc)?
What is the noble gas configuration for technetium (Tc)?
Which of the following ions is isoelectronic with argon (Ar)?
Which of the following ions is isoelectronic with argon (Ar)?
What would be the noble gas configuration of $Rb^+$?
What would be the noble gas configuration of $Rb^+$?
Who is credited with arranging elements by atomic number, which resolved inconsistencies in Mendeleev's table?
Who is credited with arranging elements by atomic number, which resolved inconsistencies in Mendeleev's table?
The periodic law states that the chemical and physical properties of elements are periodic functions of what?
The periodic law states that the chemical and physical properties of elements are periodic functions of what?
What is the significance of valence electrons in determining the properties of an element?
What is the significance of valence electrons in determining the properties of an element?
Why does atomic radius generally increase when moving down a group of elements?
Why does atomic radius generally increase when moving down a group of elements?
Considering only nitrogen (N), phosphorus (P), and arsenic (As), which atom is the largest?
Considering only nitrogen (N), phosphorus (P), and arsenic (As), which atom is the largest?
Which element requires more energy to remove its first electron: sodium (Na) or aluminum (Al)?
Which element requires more energy to remove its first electron: sodium (Na) or aluminum (Al)?
How does the first ionization energy generally change as you move from left to right across a period on the periodic table?
How does the first ionization energy generally change as you move from left to right across a period on the periodic table?
Which of the following orders of first ionization energy is correct?
Which of the following orders of first ionization energy is correct?
Why is the third ionization energy of magnesium (Mg) significantly higher than its second ionization energy?
Why is the third ionization energy of magnesium (Mg) significantly higher than its second ionization energy?
Considering chlorine (Cl), potassium (K), and zinc (Zn), which list correctly orders these atoms from highest to lowest electronegativity?
Considering chlorine (Cl), potassium (K), and zinc (Zn), which list correctly orders these atoms from highest to lowest electronegativity?
Which of the following options correctly identifies the smallest species?
Which of the following options correctly identifies the smallest species?
Flashcards
Orbital
Orbital
Region of space around the nucleus where an electron is likely to be found.
Sublevel
Sublevel
A grouping of orbitals with similar energy levels within an electron shell.
Aufbau Principle
Aufbau Principle
Electrons fill the lowest energy levels/orbitals first.
Hund's Rule
Hund's Rule
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Pauli Exclusion Principle
Pauli Exclusion Principle
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s sublevel
s sublevel
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p sublevel
p sublevel
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d sublevel
d sublevel
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Orbital Notation
Orbital Notation
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Electron Configuration
Electron Configuration
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Valence Electrons
Valence Electrons
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Bohr Model
Bohr Model
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Argon Orbital Notation
Argon Orbital Notation
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Selenium Orbital Notation
Selenium Orbital Notation
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Tin Orbital Notation
Tin Orbital Notation
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Isoelectronic
Isoelectronic
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Dmitri Mendeleev
Dmitri Mendeleev
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Mendeleev's Empty Spaces
Mendeleev's Empty Spaces
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Henry Moseley
Henry Moseley
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Periodic Law
Periodic Law
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Groups
Groups
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Periods
Periods
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Atomic Radius
Atomic Radius
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Ionization Energy
Ionization Energy
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Ionization Energy Trend (Period)
Ionization Energy Trend (Period)
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Ionization Energy Trend (Group)
Ionization Energy Trend (Group)
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Electronegativity
Electronegativity
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Electronegativity Trend (Group)
Electronegativity Trend (Group)
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Most Electronegative Element
Most Electronegative Element
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Alkali Metal Reactivity
Alkali Metal Reactivity
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Periodic Group Similarity
Periodic Group Similarity
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Periodic Period Similarity
Periodic Period Similarity
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Elements in s and p block
Elements in s and p block
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Period with 32 elements
Period with 32 elements
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Valence Electrons in Group 17
Valence Electrons in Group 17
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Valence Electrons Calculation
Valence Electrons Calculation
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Metals vs Nonmetals
Metals vs Nonmetals
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Reactive Groups
Reactive Groups
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Study Notes
- Study notes on Electron Configuration, Periodic Table Trends, and Periodic Table
Sublevels & Orbitals
- The sublevels are listed with the correct number of maximum electrons per sublevel: s2, p6, d10, f14.
- The d sublevel has 5 orbitals.
- An orbital in any sublevel can occupy a maximum of two electrons if they have opposite spins
- The fourth energy level needs 32 electrons to be completely filled.
- Number of orbitals for sublevels: s sublevel is 1, p sublevel is 3, d sublevel is 5, f sublevel is 7
- The maximum number of electrons for sublevels: s sublevel is 2, p sublevel is 6, d sublevel is 10, f sublevel is 14
- 3f orbital can never exist according to quantum theory
- The sublevel associated with a spherical (ball shaped) electron cloud identified as the "s sublevel"
Principles that Govern Electron Configuration
- The Aufbau Principle governs electron configuration: Electrons fill the lowest energy levels first.
- Hund's Rule is the rule that orbitals complete with single electrons before pairing up electrons in a single orbital
- Pauli Exclusion Principle governs the spin, two electrons can share an orbital if they have opposite spin.
- 3p4 electron should show an opposite spin, due to the Pauli Exclusion Principle
- The last electron should go in the 2nd orbital, and not paired in the 1st as described by Hund's Rule
- The 3s2 energy level should be completed before filling the 3p orbital according to the Aufbau Principle.
Orbital Notation
- Carbon's orbital notation is shown in a.
- Phosphorus is the element with orbital notation b.
Bohr Model
- Dmitri Mendeleev is attributed with arranging elements by chemical and physical properties
- Henry Moseley arranged the periodic table of elements in order of atomic number
- Scientist above predicted undiscovered elements would fill the empty spaces
- Periodic law states repetition of physical/chemical properties of elements when arranged in order of increasing atomic number
The Periodic Table
- Groups are vertical columns in the periodic table
- Each period in the periodic table corresponds to an energy level.
- Valence electrons are electrons found in the outermost energy level of atoms.
- Periods are horizontal rows in the periodic table.
- Elements in the same periodic group have the same valence configuration, valence electrons, and similar chemical properties
- Elements in the same period have the same number of occupied energy levels.
- A period where only s and p sublevels are filled has 8 elements.
- A period containing 32 elements contains the sublevels s, p, d, f.
- Group 17 elements have 7 valence electrons
- For groups 13-18, valence electrons equals the group number minus 10
- Group 2 elements have valence electrons in the s sublevel.
Elements, Classes, and Families
- Three classes of elements: metals, nonmetals, and metalloids
- A on the table represents metals
- B on the table represents metalloids
- C on the ble represents nonmetals
- Element in period 5, group 14: tin, Sn
- Element in period 3, group 17: chlorine, Cl
- Element in period 6, group 2: barium, Ba
Periodic Trends
- Metals lose electrons, are good conductors, and are malleable and ductile
- Nonmetals gain electrons, are brittle and dull, and are not conductors
- Most reactive nonmetals belong to group 17: halogens
- Group 18 elements are unreactive (noble gases)
- The family termed "basic" are group 2: alkaline earth metals
- Groups 3-12 are transition metals, and are also metals
- The most reactive metals are groups 1: alkali metals
- Actinides are elements in the second row of the f-block
- Metalloids have both metallic and nonmetallic properties
- Atomic radius decreases across the periodic table because the number of protons in the nucleus increases and pulls the electrons closer
- Atomic radius generally increases moving down a group because the number of occupied energy levels increases
- Arsenic is the largest of the following: nitrogen, phosphorus, or arsenic
- Phosphorus is the largest atom out of phosphorus, sulfur and chlorine on the periodic table
- Fluorine is the smallest atom out of nitrogen, oxygen and fluorine
- Ionization energy is the energy needed to remove one electron from an atom
- Aluminum requires more energy than sodium to remove its first electron.
- First ionization energies increase moving left to right across a period.
- Moving from top to bottom of a group, first ionization energies decrease.
- Of the choices below, which gives the correct order of ionization energy? Cl > S > P > Si > Al
- Phosphorus has the highest ionization energy of aluminum, silicon and phosphorus.
- The third ionization energy of magnesium is greater because magnesium will achieve a full octet for its outer energy level
- Sulfur has the highest ionization energy of tin, arsenic, and sulfur
- Decreasing electronegativity: chlorine, zinc, potassium (Cl, Zn, K)
- Electronegativity decreases moving down the periodic table.
- Fluorine is the most electronegative element
- Metals tend to have low electronegativity.
- Of the following, the smallest is a lithium ion
- Of the following, K+ will have a larger radius than K or Ca2+
- Reactivity increases going down group 1 and decreases going down group 17
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