Chemistry Chapter 6: The Periodic Table

Choose a study mode

Play Quiz
Study Flashcards
Spaced Repetition
Chat to Lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

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?

  • 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?

  • Henry Moseley (correct)
  • John Newlands
  • Dmitri Mendeleev
  • Lavoisier

What was one significant observation made by John Newlands about elements ordered by increasing atomic mass?

<p>Their properties repeat every eighth element (A)</p> Signup and view all the answers

Which of the following elements is classified as a metalloid?

<p>Silicon (D)</p> Signup and view all the answers

What information is contained in each box of the modern periodic table?

<p>Element's name, symbol, atomic number, and atomic mass (A)</p> Signup and view all the answers

What defines why elements in the same group have similar properties?

<p>Their electron configurations (C)</p> Signup and view all the answers

Which of the following is true regarding nonmetals?

<p>They are generally gases or brittle solids. (A)</p> Signup and view all the answers

Which term describes the columns of elements in the periodic table?

<p>Groups (A)</p> Signup and view all the answers

Which groups of elements are classified as alkali metals?

<p>Group 1 (B)</p> Signup and view all the answers

What are the elements in groups 3 to 12 known as?

<p>Transition metals (D)</p> Signup and view all the answers

What is the term for elements such as lithium and sodium, which belong to the same group?

<p>Alkali metals (B)</p> Signup and view all the answers

In which century did Lavoisier compile a list of known elements?

<p>18th century (B)</p> Signup and view all the answers

What key feature did Meyer and Mendeleev reveal about the relationship between atomic mass and elements?

<p>There is a clear connection between atomic mass and elemental properties (C)</p> Signup and view all the answers

What is the significance of valence electrons in determining an element's position on the periodic table?

<p>They indicate the period and group of the element (C)</p> Signup and view all the answers

What elements make up the alkaline earth metals?

<p>Elements in group 2 of the periodic table (A)</p> Signup and view all the answers

What is the group number of strontium based on its electron configuration [Kr]5s2?

<p>2 (A)</p> Signup and view all the answers

What defines the halogens on the periodic table?

<p>Highly reactive elements in group 17 (A)</p> Signup and view all the answers

What characterizes the s-block of the periodic table?

<p>Elements in group 1 and group 2 along with helium (D)</p> Signup and view all the answers

How many valence electrons do the elements in group 2 possess?

<p>Two (B)</p> Signup and view all the answers

Which of the following pairs are classified as metalloids?

<p>Silicon and germanium (B)</p> Signup and view all the answers

What happens to the electrons in the groups from 13 to 18 regarding their valence electrons?

<p>They decrease by ten less than their group number (D)</p> Signup and view all the answers

What distinguishes inner transition metals from transition metals?

<p>They are divided into lanthanides and actinides. (B)</p> Signup and view all the answers

Which group contains noble gases?

<p>Group 18 (A)</p> Signup and view all the answers

Which of the following elements is in the d-block?

<p>Iron (Fe) (A)</p> Signup and view all the answers

How many groups does the f-block span on the periodic table?

<p>14 (C)</p> Signup and view all the answers

What is the maximum number of electrons that can occupy the d orbitals in an element?

<p>10 (B)</p> Signup and view all the answers

Which of the following blocks contains the transition metals?

<p>d-block (B)</p> Signup and view all the answers

Which of the following statements about d-block elements is TRUE?

<p>They have completely filled or partially filled d orbitals. (C)</p> Signup and view all the answers

What is the period number of an element with the electron configuration [Xe]6s24f145d106p3?

<p>6 (D)</p> Signup and view all the answers

Which statement correctly describes the relationship between electron configuration and the position of an element on the periodic table?

<p>The highest energy level of the electrons determines the period number. (A)</p> Signup and view all the answers

Why do elements in the same group have similar chemical properties?

<p>They have the same number of valence electrons. (A)</p> Signup and view all the answers

What happens to the atomic radius as the principal orbital increases?

<p>It increases as outer electrons are farther from the nucleus. (C)</p> Signup and view all the answers

Which element has the largest atomic radius in period 2?

<p>Lithium (Li) (A)</p> Signup and view all the answers

Why do positively charged ions typically have a smaller radius than their neutral atoms?

<p>They lose valence electrons, which can empty outer orbitals. (D)</p> Signup and view all the answers

What is one reason the atomic radius decreases across a period?

<p>Electrons are pulled closer to the nucleus by increased nuclear charge. (A)</p> Signup and view all the answers

What role does electrostatic repulsion play in ionic radius?

<p>It decreases and allows electrons to be pulled closer. (D)</p> Signup and view all the answers

Which factor contributes to the shielding effect on outer electrons?

<p>The presence of additional orbitals between nucleus and electrons. (C)</p> Signup and view all the answers

What effect does losing a valence electron have on an atom's radius?

<p>The radius decreases due to reduced electron-electron repulsion. (B)</p> Signup and view all the answers

As you move from beryllium to fluorine in period 2, what trend is observed?

<p>The atomic radius decreases. (D)</p> Signup and view all the answers

What are the four blocks of the periodic table based on electron configurations?

<p>s, p, d, f (D)</p> Signup and view all the answers

How does atomic radius generally change as you move from left to right across a period?

<p>Decreases due to increasing nuclear charge (C)</p> Signup and view all the answers

What causes the atomic radius to increase as you move down a group in the periodic table?

<p>Increase in outermost orbital size (D)</p> Signup and view all the answers

Which of the following correctly identifies the role of strong nuclear force?

<p>Binding nucleons together in the nucleus (A)</p> Signup and view all the answers

Which of the following correctly describes the concept of electronegativity?

<p>The tendency of an atom to attract electrons (B)</p> Signup and view all the answers

What is the definition of atomic radius for elements that occur as molecules?

<p>Half the distance between the nuclei of identical atoms that are chemically bonded (C)</p> Signup and view all the answers

Which force is responsible for the electrostatic repulsion experienced between protons in the nucleus?

<p>Electrostatic force (A)</p> Signup and view all the answers

What is the relationship between atomic radius and electron configuration?

<p>Atomic radius is influenced by the distribution of electrons in principal energy levels (C)</p> Signup and view all the answers

Flashcards

Periodic Table

An arrangement of elements based on increasing atomic number and recurring properties.

Atomic Number

The number of protons in the nucleus of an atom, unique to each element.

Periodic Law

The principle that the properties of elements repeat in a predictable way when arranged by atomic number.

Lavoisier

A scientist who compiled a list of known elements in the 1700s.

Signup and view all the flashcards

Mendeleev

A scientist who created an early periodic table based on atomic mass, predicting undiscovered elements.

Signup and view all the flashcards

Moseley

A scientist who rearranged the periodic table by increasing atomic number, clarifying properties.

Signup and view all the flashcards

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

A series of 15 elements from lanthanum to lutetium, known for unique properties and uses.

Signup and view all the flashcards

Modern Periodic Table

A table organizing elements by atomic number, symbol, and properties.

Signup and view all the flashcards

Groups

Columns in the periodic table that contain elements with similar properties.

Signup and view all the flashcards

Periods

Rows in the periodic table representing energy levels of electrons.

Signup and view all the flashcards

Representative Elements

Elements in groups 1-2 and 13-18 with varied properties.

Signup and view all the flashcards

Transition Metals

Elements in groups 3-12 known for their ability to conduct electricity.

Signup and view all the flashcards

Alkali Metals

Highly reactive metals in group 1, excluding hydrogen.

Signup and view all the flashcards

Halogens

Group 17 elements that are highly reactive and form salts with metals.

Signup and view all the flashcards

Noble Gases

Unreactive gases in group 18, known for stability.

Signup and view all the flashcards

Valence Electrons

Electrons in the highest principal energy level of an atom.

Signup and view all the flashcards

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

Elements in groups 13 to 18 where p orbitals are filled.

Signup and view all the flashcards

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

The four blocks are s, p, d, and f based on electron configurations.

Signup and view all the flashcards

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

Atomic radius decreases left to right and increases top to bottom in the periodic table.

Signup and view all the flashcards

Ionization Energy

The energy required to remove an electron from an atom in its gaseous state.

Signup and view all the flashcards

Electronegativity

A measure of an atom's ability to attract and hold onto electrons.

Signup and view all the flashcards

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

The force that binds protons and neutrons together in the nucleus, providing stability.

Signup and view all the flashcards

Shielding Effect

Reduction of the effective nuclear charge felt by valence electrons due to inner electrons.

Signup and view all the flashcards

Electron Configuration

The arrangement of electrons in an atom's orbitals.

Signup and view all the flashcards

Group Number

The column number in the periodic table indicating elements with similar properties.

Signup and view all the flashcards

Period Number

The row number in the periodic table indicating the highest energy level.

Signup and view all the flashcards

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

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 generally increases down a group and decreases across a period from left to right.

Signup and view all the flashcards

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

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

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

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

The force that attracts electrons towards the positively charged nucleus, stronger in smaller ions.

Signup and view all the flashcards

Study 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.
  • 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.

Quiz Team

Related Documents

Chapter 6 The Periodic Table PDF

More Like This

Use Quizgecko on...
Browser
Open
Browser
Browser