Chemistry Chapter 5 Flashcards
58 Questions
100 Views

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

Who was Dmitri Mendeleev?

The Father of the Periodic Table

How did he classify the elements on the Periodic Table?

By arranging them according to increasing atomic mass.

How does Mendeleev's periodic table compare to our present version?

It was organized by mass numbers, not atomic numbers.

What did Henry Moseley discover?

<p>A pattern of elements fit better when arranged by atomic number.</p> Signup and view all the answers

What is the Periodic Law?

<p>The physical and chemical properties of the elements are periodic functions of their atomic number.</p> Signup and view all the answers

What is the Periodic Table?

<p>An arrangement of the elements in order of their atomic numbers.</p> Signup and view all the answers

What are the noble gases?

<p>Chemically unreactive gases located in the last vertical column of the periodic table.</p> Signup and view all the answers

What are the lanthanides?

<p>The fourteen elements with atomic numbers ranging from 58 to 71.</p> Signup and view all the answers

What are the actinides?

<p>The fourteen elements ranging from atomic number 90 to 103.</p> Signup and view all the answers

What do we mean by periodicity?

<p>Repeatable properties and characteristics.</p> Signup and view all the answers

What are the horizontal rows of the periodic table called?

<p>Periods.</p> Signup and view all the answers

What is the same as the number of the period?

<p>The number of principal energy levels being filled.</p> Signup and view all the answers

What are the vertical columns of the periodic table called?

<p>Groups or families.</p> Signup and view all the answers

Where are the metals found on the Periodic Table?

<p>To the left of the staircase.</p> Signup and view all the answers

What names are given to some groups of metals?

<p>Group IA is called alkali metals, and Group IIA is called alkaline earth metals.</p> Signup and view all the answers

Which group contains the most active metals?

<p>Alkali metals.</p> Signup and view all the answers

What are some physical and chemical properties of metals?

<p>Good conductors of heat and electricity; shiny; malleable; ductile; mostly solid.</p> Signup and view all the answers

Where are the nonmetals found on the periodic table?

<p>To the right of the staircase.</p> Signup and view all the answers

Which group contains the most active nonmetals?

<p>Group VIIA, halogens.</p> Signup and view all the answers

What names are given to groups of nonmetals?

<p>Group VIA is called chalcogens, Group VIIA is called halogens, and Group VIIIA is called noble gases.</p> Signup and view all the answers

What are some physical and chemical properties of nonmetals?

<p>Insulators; dull; brittle; not malleable or ductile; mostly gaseous.</p> Signup and view all the answers

What is a metalloid?

<p>An element that has properties of both metals and nonmetals.</p> Signup and view all the answers

Give some examples of metalloids.

<p>Boron, silicon, germanium, arsenic, antimony, tellurium, polonium, and astatine.</p> Signup and view all the answers

Where are the transition elements found on the periodic table?

<p>In the middle of the periodic table from groups 3 to 12.</p> Signup and view all the answers

What characteristics of atomic structure distinguish the transition elements from the main group elements?

<p>They have unfilled 'd' orbitals in their electron configurations.</p> Signup and view all the answers

Why are the elements of group VIIIA or Group O called the noble or inert gases?

<p>They are very unreactive due to their completely filled outer energy levels.</p> Signup and view all the answers

What is atomic radius?

<p>One-half the distance between the nuclei of bonded atoms.</p> Signup and view all the answers

What is the trend for atomic radius when going down a group on the Periodic Table?

<p>Atomic radius increases due to an increase in the number of energy levels.</p> Signup and view all the answers

Why does this trend occur?

<p>More energy levels lead to a larger atomic size.</p> Signup and view all the answers

What is the trend for atomic radius when going across a period?

<p>It decreases as the nucleus gets larger and attracts electrons.</p> Signup and view all the answers

What is an ion?

<p>A charged atom formed by the gain or loss of electrons.</p> Signup and view all the answers

What is ionization?

<p>Any process that results in the formation of an ion.</p> Signup and view all the answers

What is ionization energy?

<p>The energy required to remove one electron from a neutral atom.</p> Signup and view all the answers

What is the trend for ionization energy when going down a group on the Periodic Table?

<p>Ionization energy generally decreases.</p> Signup and view all the answers

Why does this trend occur?

<p>Electrons are far from the nucleus and can be more easily removed.</p> Signup and view all the answers

What is the trend for ionization energy going across a period?

<p>Ionization energy generally increases.</p> Signup and view all the answers

Why does this trend occur?

<p>More nuclear charge attracts electrons more strongly.</p> Signup and view all the answers

What is the trend for successive ionization energies?

<p>Each successive ionization energy is higher than the first.</p> Signup and view all the answers

What is electron affinity?

<p>The energy change that occurs when an electron is acquired by a neutral atom.</p> Signup and view all the answers

What are the trends for electron affinity on the periodic table?

<p>It increases going across a period and decreases down a group.</p> Signup and view all the answers

Why do these trends occur?

<p>Atoms that want to gain electrons to achieve stability.</p> Signup and view all the answers

What is a cation?

<p>A positive ion.</p> Signup and view all the answers

What is an anion?

<p>A negative ion.</p> Signup and view all the answers

What is the trend for ionic radius on the periodic table?

<p>Ionic radii of metals are smaller than atomic radii, while nonmetals have larger ionic radii.</p> Signup and view all the answers

What are valence electrons?

<p>Electrons in the outermost energy level of an atom.</p> Signup and view all the answers

What is electronegativity?

<p>A measure of the ability of an atom in a chemical compound to attract electrons.</p> Signup and view all the answers

What is the trend for electronegativity when going across a period on the Periodic Table?

<p>Electronegativity increases.</p> Signup and view all the answers

Why does this trend occur?

<p>Going toward nonmetals that want to gain electrons.</p> Signup and view all the answers

What is the trend for electronegativity when going down a group on the Periodic Table?

<p>Electronegativity decreases.</p> Signup and view all the answers

Why does this trend occur?

<p>Smaller atoms are better at pulling electrons in.</p> Signup and view all the answers

What is the 's' block?

<p>Groups 1 and 2 on the Periodic Table.</p> Signup and view all the answers

What are some characteristics of the elements found in the 's' block?

<p>Active metals with +1/+2 oxidation states that form basic oxides.</p> Signup and view all the answers

What is the 'p' block of elements?

<p>Elements found in Groups 13 - 18 on the Periodic Table.</p> Signup and view all the answers

What are some characteristics of the elements found in the 'p' block?

<p>Most are nonmetals with variable oxidation states that form acidic oxides.</p> Signup and view all the answers

What is the 'd' block of elements?

<p>Groups 3 - 12 on the Periodic Table.</p> Signup and view all the answers

What are some characteristics of these elements?

<p>d-block elements exhibit variable oxidation states and form colored compounds.</p> Signup and view all the answers

What is the 'f' block of elements?

<p>Elements # 58 - 71 and # 90 - 103.</p> Signup and view all the answers

What are some characteristics of these elements?

<p>Lanthanides and actinides show similar chemical properties and include radioactive elements.</p> Signup and view all the answers

Study Notes

Dmitri Mendeleev and the Periodic Table

  • Dmitri Mendeleev is recognized as the "Father of the Periodic Table" for organizing elements by their properties.
  • He utilized cards to categorize elements based on atomic mass and characteristics, revealing periodic patterns.

Classification of Elements

  • Mendeleev classified elements by increasing atomic mass, leading to regular similarities in chemical and physical properties.
  • His early periodic table was arranged by mass numbers instead of atomic numbers, which was a key distinction from modern tables.

Discovery by Henry Moseley

  • Henry Moseley discovered that arranging elements by atomic number revealed a clearer pattern among them.
  • This revelation established the modern periodic law.

Periodic Law and Table

  • The Periodic Law states that the physical and chemical properties of elements are functions of their atomic number, with similar properties appearing at regular intervals.
  • The current Periodic Table organizes elements by atomic number, grouping those with similar properties in columns.

Noble Gases and Specific Element Groups

  • Noble gases, found in the last vertical column, include helium, neon, argon, krypton, xenon, and radon, known for their chemical inertness.
  • Lanthanides are elements with atomic numbers 58 to 71, while actinides range from atomic numbers 90 to 103.

Periodicity

  • Periodicity refers to the repeatable properties observed in groups on the periodic table due to electron arrangements.
  • Horizontal rows are labeled periods, corresponding to the number of principal energy levels filled.

Metals, Nonmetals, and Metalloids

  • Metals, located left of the staircase on the table, include alkali metals (Group IA) and alkaline earth metals (Group IIA).
  • Nonmetals are to the right of the staircase, including halogens (Group VIIA) and noble gases (Group VIIIA).
  • Metalloids share properties of both metals and nonmetals, positioned along the staircase.

Transition Elements

  • Transition elements, found in the middle (Groups 3-12), exhibit unique properties due to unfilled d orbitals and can form various ion charges.
  • Atomic radius measures half the distance between nuclei of bonded atoms, influenced by energy levels.
  • Atomic radius decreases across a period (increased nucleus attraction) and increases down a group (more energy levels).

Ionization and Ionic Properties

  • Ionization refers to the formation of charged ions through electron gain/loss.
  • Ionization energy decreases down a group (increased distance from nucleus) and increases across a period (higher nuclear charge).
  • Cations are positively charged ions, while anions are negatively charged ions.

Valence Electrons and Electronegativity

  • Valence electrons in the outermost energy level dictate chemical behavior and bonding capacity, with their count relating to group numbers.
  • Electronegativity, indicating an atom's ability to attract electrons, increases across a period and decreases down a group, with fluorine being the highest.

Element Blocks in the Periodic Table

  • The "s" block contains Groups 1 and 2, primarily active metals with +1 or +2 oxidation states.
  • The "p" block includes Groups 13-18, which mainly consist of non-metals, variable oxidation states, and acidic oxides.
  • The "d" block (Groups 3-12) features transition metals known for variable oxidation states and colorful compounds.
  • The "f" block (lanthanides and actinides) consists of inner transition elements with special properties such as radioactivity and unique chemical behaviors.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Quiz Team

Description

This quiz covers key concepts from Chemistry Chapter 5, focusing on Dmitri Mendeleev and his contributions to the Periodic Table. It includes essential terms and definitions that explain how elements are classified. Perfect for reinforcing your understanding of atomic mass and the organization of elements.

More Like This

Use Quizgecko on...
Browser
Open
Browser
Browser