Podcast
Questions and Answers
What arrangement did John Newlands propose for organizing elements?
What arrangement did John Newlands propose for organizing elements?
- By their chemical reactivity
- By their atomic radius
- By increasing atomic number
- By increasing atomic mass (correct)
What is known as the periodic law?
What is known as the periodic law?
- The law stating all metals are solid at room temperature
- The classification of elements solely based on their state of matter
- The repetition of properties when elements are arranged by increasing atomic mass
- The periodic repetition of chemical and physical properties when elements are arranged by increasing atomic number (correct)
Which scientist is credited with rearranging the periodic table by increasing atomic number?
Which scientist is credited with rearranging the periodic table by increasing atomic number?
- Henry Moseley (correct)
- John Newlands
- Dmitri Mendeleev
- Lavoisier
What was one significant observation made by John Newlands about elements ordered by increasing atomic mass?
What was one significant observation made by John Newlands about elements ordered by increasing atomic mass?
Which of the following elements is classified as a metalloid?
Which of the following elements is classified as a metalloid?
What information is contained in each box of the modern periodic table?
What information is contained in each box of the modern periodic table?
What defines why elements in the same group have similar properties?
What defines why elements in the same group have similar properties?
Which of the following is true regarding nonmetals?
Which of the following is true regarding nonmetals?
Which term describes the columns of elements in the periodic table?
Which term describes the columns of elements in the periodic table?
Which groups of elements are classified as alkali metals?
Which groups of elements are classified as alkali metals?
What are the elements in groups 3 to 12 known as?
What are the elements in groups 3 to 12 known as?
What is the term for elements such as lithium and sodium, which belong to the same group?
What is the term for elements such as lithium and sodium, which belong to the same group?
In which century did Lavoisier compile a list of known elements?
In which century did Lavoisier compile a list of known elements?
What key feature did Meyer and Mendeleev reveal about the relationship between atomic mass and elements?
What key feature did Meyer and Mendeleev reveal about the relationship between atomic mass and elements?
What is the significance of valence electrons in determining an element's position on the periodic table?
What is the significance of valence electrons in determining an element's position on the periodic table?
What elements make up the alkaline earth metals?
What elements make up the alkaline earth metals?
What is the group number of strontium based on its electron configuration [Kr]5s2?
What is the group number of strontium based on its electron configuration [Kr]5s2?
What defines the halogens on the periodic table?
What defines the halogens on the periodic table?
What characterizes the s-block of the periodic table?
What characterizes the s-block of the periodic table?
How many valence electrons do the elements in group 2 possess?
How many valence electrons do the elements in group 2 possess?
Which of the following pairs are classified as metalloids?
Which of the following pairs are classified as metalloids?
What happens to the electrons in the groups from 13 to 18 regarding their valence electrons?
What happens to the electrons in the groups from 13 to 18 regarding their valence electrons?
What distinguishes inner transition metals from transition metals?
What distinguishes inner transition metals from transition metals?
Which group contains noble gases?
Which group contains noble gases?
Which of the following elements is in the d-block?
Which of the following elements is in the d-block?
How many groups does the f-block span on the periodic table?
How many groups does the f-block span on the periodic table?
What is the maximum number of electrons that can occupy the d orbitals in an element?
What is the maximum number of electrons that can occupy the d orbitals in an element?
Which of the following blocks contains the transition metals?
Which of the following blocks contains the transition metals?
Which of the following statements about d-block elements is TRUE?
Which of the following statements about d-block elements is TRUE?
What is the period number of an element with the electron configuration [Xe]6s24f145d106p3?
What is the period number of an element with the electron configuration [Xe]6s24f145d106p3?
Which statement correctly describes the relationship between electron configuration and the position of an element on the periodic table?
Which statement correctly describes the relationship between electron configuration and the position of an element on the periodic table?
Why do elements in the same group have similar chemical properties?
Why do elements in the same group have similar chemical properties?
What happens to the atomic radius as the principal orbital increases?
What happens to the atomic radius as the principal orbital increases?
Which element has the largest atomic radius in period 2?
Which element has the largest atomic radius in period 2?
Why do positively charged ions typically have a smaller radius than their neutral atoms?
Why do positively charged ions typically have a smaller radius than their neutral atoms?
What is one reason the atomic radius decreases across a period?
What is one reason the atomic radius decreases across a period?
What role does electrostatic repulsion play in ionic radius?
What role does electrostatic repulsion play in ionic radius?
Which factor contributes to the shielding effect on outer electrons?
Which factor contributes to the shielding effect on outer electrons?
What effect does losing a valence electron have on an atom's radius?
What effect does losing a valence electron have on an atom's radius?
As you move from beryllium to fluorine in period 2, what trend is observed?
As you move from beryllium to fluorine in period 2, what trend is observed?
What are the four blocks of the periodic table based on electron configurations?
What are the four blocks of the periodic table based on electron configurations?
How does atomic radius generally change as you move from left to right across a period?
How does atomic radius generally change as you move from left to right across a period?
What causes the atomic radius to increase as you move down a group in the periodic table?
What causes the atomic radius to increase as you move down a group in the periodic table?
Which of the following correctly identifies the role of strong nuclear force?
Which of the following correctly identifies the role of strong nuclear force?
Which of the following correctly describes the concept of electronegativity?
Which of the following correctly describes the concept of electronegativity?
What is the definition of atomic radius for elements that occur as molecules?
What is the definition of atomic radius for elements that occur as molecules?
Which force is responsible for the electrostatic repulsion experienced between protons in the nucleus?
Which force is responsible for the electrostatic repulsion experienced between protons in the nucleus?
What is the relationship between atomic radius and electron configuration?
What is the relationship between atomic radius and electron configuration?
Flashcards
Periodic Table
Periodic Table
An arrangement of elements based on increasing atomic number and recurring properties.
Atomic Number
Atomic Number
The number of protons in the nucleus of an atom, unique to each element.
Periodic Law
Periodic Law
The principle that the properties of elements repeat in a predictable way when arranged by atomic number.
Lavoisier
Lavoisier
A scientist who compiled a list of known elements in the 1700s.
Signup and view all the flashcards
Mendeleev
Mendeleev
A scientist who created an early periodic table based on atomic mass, predicting undiscovered elements.
Signup and view all the flashcards
Moseley
Moseley
A scientist who rearranged the periodic table by increasing atomic number, clarifying properties.
Signup and view all the flashcards
Alkaline Earth Metals
Alkaline Earth Metals
A group of metals in Group 2 of the periodic table, reactive but less than alkali metals.
Signup and view all the flashcards
Lanthanide Series
Lanthanide Series
A series of 15 elements from lanthanum to lutetium, known for unique properties and uses.
Signup and view all the flashcards
Modern Periodic Table
Modern Periodic Table
A table organizing elements by atomic number, symbol, and properties.
Signup and view all the flashcards
Groups
Groups
Columns in the periodic table that contain elements with similar properties.
Signup and view all the flashcards
Periods
Periods
Rows in the periodic table representing energy levels of electrons.
Signup and view all the flashcards
Representative Elements
Representative Elements
Elements in groups 1-2 and 13-18 with varied properties.
Signup and view all the flashcards
Transition Metals
Transition Metals
Elements in groups 3-12 known for their ability to conduct electricity.
Signup and view all the flashcards
Alkali Metals
Alkali Metals
Highly reactive metals in group 1, excluding hydrogen.
Signup and view all the flashcards
Halogens
Halogens
Group 17 elements that are highly reactive and form salts with metals.
Signup and view all the flashcards
Noble Gases
Noble Gases
Unreactive gases in group 18, known for stability.
Signup and view all the flashcards
Valence Electrons
Valence Electrons
Electrons in the highest principal energy level of an atom.
Signup and view all the flashcards
s-block Elements
s-block Elements
Elements in groups 1, 2, and helium with partially or completely filled s orbitals.
Signup and view all the flashcards
p-block Elements
p-block Elements
Elements in groups 13 to 18 where p orbitals are filled.
Signup and view all the flashcards
Inner Transition Metals
Inner Transition Metals
The lanthanide and actinide series found at the bottom of the periodic table.
Signup and view all the flashcards
Blocks of the Periodic Table
Blocks of the Periodic Table
The four blocks are s, p, d, and f based on electron configurations.
Signup and view all the flashcards
Atomic Radius
Atomic Radius
The atomic radius is the distance from the nucleus to the outermost electron shell.
Signup and view all the flashcards
Trends in Atomic Radius
Trends in Atomic Radius
Atomic radius decreases left to right and increases top to bottom in the periodic table.
Signup and view all the flashcards
Ionization Energy
Ionization Energy
The energy required to remove an electron from an atom in its gaseous state.
Signup and view all the flashcards
Electronegativity
Electronegativity
A measure of an atom's ability to attract and hold onto electrons.
Signup and view all the flashcards
Electrostatic Force
Electrostatic Force
The force of attraction between protons and electrons in an atom, varies with distance.
Signup and view all the flashcards
Strong Nuclear Force
Strong Nuclear Force
The force that binds protons and neutrons together in the nucleus, providing stability.
Signup and view all the flashcards
Shielding Effect
Shielding Effect
Reduction of the effective nuclear charge felt by valence electrons due to inner electrons.
Signup and view all the flashcards
Electron Configuration
Electron Configuration
The arrangement of electrons in an atom's orbitals.
Signup and view all the flashcards
Group Number
Group Number
The column number in the periodic table indicating elements with similar properties.
Signup and view all the flashcards
Period Number
Period Number
The row number in the periodic table indicating the highest energy level.
Signup and view all the flashcards
s-block
s-block
The first two groups of the periodic table where the outermost electrons are in the s orbital.
Signup and view all the flashcards
Principal Orbital
Principal Orbital
The main energy level of electrons in an atom, which increases with distance from the nucleus.
Signup and view all the flashcards
Atomic Radius Trend
Atomic Radius Trend
Atomic radius generally increases down a group and decreases across a period from left to right.
Signup and view all the flashcards
Largest Atomic Radius (Example)
Largest Atomic Radius (Example)
Among Li, Be, C, and F, Li has the largest atomic radius due to its position in the period.
Signup and view all the flashcards
Ionic Radius
Ionic Radius
The radius of an atom's ion which can differ from its atomic radius, depending on gain or loss of electrons.
Signup and view all the flashcards
Cation Size Change
Cation Size Change
When an atom loses electrons to form a cation, the ionic radius decreases due to less electron-electron repulsion.
Signup and view all the flashcards
Anion Size Change
Anion Size Change
When an atom gains electrons to form an anion, the ionic radius increases due to increased repulsion.
Signup and view all the flashcards
Electrostatic Attraction
Electrostatic Attraction
The force that attracts electrons towards the positively charged nucleus, stronger in smaller ions.
Signup and view all the flashcardsStudy Notes
Chapter 6: The Periodic Table
- The periodic table organizes elements based on their properties.
- Arrangement is based on increasing atomic number.
- Elements with similar properties are grouped together.
Section 1: Development of the Modern Periodic Table
- Scientists in the 1700's attempted to organize known elements.
- Lavoisier created a list of known elements.
- In the 1800's, John Newlands attempted to arrange elements by increasing atomic mass.
- He noticed a repeating pattern of properties every 8th element (Law of Octaves).
- Lothar Meyer demonstrated a connection between atomic mass and properties of elements.
- Dmitri Mendeleev arranged elements by increasing atomic mass and left gaps for undiscovered elements.
- Henry Moseley rearranged the periodic table by increasing atomic number.
- This arrangement resulted in a clear periodic pattern (Periodic Law).
Vocabulary
- atomic number: The number of protons in an atom's nucleus.
- periodic law: The properties of elements repeat in a periodic pattern when arranged by increasing atomic number.
- group: A column on the periodic table. Elements in the same group exhibit similar chemical properties.
- period: A row on the periodic table. Elements in the same period show trends in properties.
- representative element: Elements in groups 1, 2, and 13-18.
- transition element: Elements in groups 3-12.
- metal: Elements that are generally shiny, solid at room temperature, and good conductors of heat and electricity.
- alkali metal: Elements in group 1 (except hydrogen).
- alkaline earth metal: Elements in group 2.
- transition metal: Elements in groups 3-12.
- inner transition metal: Elements in the f-block (lanthanides and actinides).
- lanthanide series: Fourteen elements following lanthanum (in the 6th row/period).
- actinide series: Fourteen elements following actinium (in the 7th row/period).
- nonmetal: Elements that are generally gases or brittle, dull solids, and poor conductors of heat and electricity.
- halogen: Elements in group 17.
- noble gas: Elements in group 18.
- metalloid: Elements with characteristics of both metals and nonmetals.
Section 2: Classification of Elements
- Elements in the same group have similar properties due to similar electron configurations.
- The periodic table is divided into four blocks based on their electron configurations: s-block, p-block, d-block, and f-block.
- s-block elements are in groups 1 and 2 and include hydrogen and helium.
- p-block elements are in groups 13-18.
- d-block elements are transition metals.
- f-block elements are inner transition metals.
Section 3: Periodic Trends
- Atomic radius: The size of an atom. Atomic radius increases down a group and decreases across a period.
- Ionic radius: The size of an ion. Positive ions are smaller than the neutral atoms. Negative ions are larger than the neutral atoms.
- ionization energy: The energy required to remove an electron from a neutral gaseous atom. First ionization energy increases across a period and decreases down a group.
- octet rule: Atoms tend to gain, lose, or share electrons to achieve a full set of eight valence electrons.
- electronegativity: The ability of an atom to attract electrons in a chemical bond. Electronegativity generally increases across a period and decreases down a group.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
