Chemistry Chapter 5 Study Guide

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Questions and Answers

What does the term 'Periodic' refer to?

A type of chemical reaction

Repeating patterns (correct)

A specific element

None of the above

What is the Periodic Law?

The physical and chemical properties of the elements that are periodic functions of their atomic numbers.

What is the Periodic Table?

Arrangement of the elements by their properties.

What is the Modern Periodic Table?

Elements arranged in order of atomic numbers with similar properties in the same group. Signup and view all the answers

What are Lanthanides?

Atomic #'s 58-71, shiny, reactive metals with similar properties. Signup and view all the answers

What are Actinides?

Atomic #'s 90-103, radioactive metals, mostly synthesized. Signup and view all the answers

What are Periods on the Periodic Table?

The horizontal arrangement of elements. Signup and view all the answers

The blocks s, p, d, and f in the periodic table are based on the ______ configuration of elements.

electron Signup and view all the answers

Which group is known as the most reactive and soft metals?

Alkali Metals Signup and view all the answers

What are Alkaline Earth Metals known for?

They are harder, denser, stronger, and less reactive than Alkali Metals. Signup and view all the answers

What are Transition Elements?

Groups 3-12 elements that are less reactive. Signup and view all the answers

Which group includes the least reactive elements?

Noble Gases Signup and view all the answers

What is an Ion?

An atom with a positive or negative charge Signup and view all the answers

What is Ionization?

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

What is a Cation?

A positively charged ion. Signup and view all the answers

What is an Anion?

A negatively charged ion. Signup and view all the answers

Define Atomic Radii.

One-half the distance between the nuclei of identical atoms that are bonded together. Signup and view all the answers

Define Ionic Radii.

One-half the diameter of an atom's ion. Signup and view all the answers

What is Ionization Energy?

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

What is Electron Affinity?

The energy change when an electron is acquired by a neutral atom. Signup and view all the answers

Define Electronegativity.

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

Who introduced the method for accurately measuring atomic masses?

Stanislao Cannizzaro. Signup and view all the answers

Who published the first periodic table?

Dmitri Mendeleev. Signup and view all the answers

What did Henry Moseley realize about the periodic arrangement of elements?

Elements are arranged in order of increasing atomic number. Signup and view all the answers

What are Group Configurations related to?

The number of valence electrons corresponding to group numbers. Signup and view all the answers

What are Valence Electrons?

Electrons available in chemical compounds to be shared, gained, or lost. Signup and view all the answers

Study Notes

Periodic Concepts

Periodicity refers to repeating patterns in properties of elements.
The Periodic Law states properties of elements are periodic functions of their atomic numbers.
The Periodic Table organizes elements according to their properties and atomic numbers.

Modern Periodic Table

Elements are arranged by atomic number, grouping similar properties together.
Incorporates newly discovered elements including Noble Gases, Lanthanides, and Actinides since Mendeleev's time.

Lanthanides and Actinides

Lanthanides (Atomic #s 58-71): Shiny, reactive metals filling F orbitals, similar to alkaline earth metals.
Actinides (Atomic #s 90-103): Mostly synthetic, radioactive metals, with only 90-92 occurring naturally.

Structure of the Periodic Table

Periods run horizontally and their length is determined by the number of electrons in sub-levels.
The s, p, d, and f blocks correspond to electron configurations, indicative of group placement:
- s block: max 2 electrons
- p block: max 6 electrons
- d block: max 10 electrons
- f block: max 14 electrons.

Element Groups

Alkali Metals (Group 1): Highly reactive, soft silvery metals, stored under oil, rarely found in nature.
Alkaline Earth Metals (Group 2): Harder and denser than Alkali Metals, less reactive, cannot be found freely in nature.
Transition Elements (Groups 3-12): Shiny, conductive, ductile, and malleable, with less reactivity compared to Groups 1 and 2, some found as native elements.
Main Group Elements (Groups 13-18): Occupy s and p blocks, varied properties; include metals, nonmetals, and metalloids.
Halogens (Group 17): Most reactive non-metals, capable of forming salts with metals.
Noble Gases (Group 18): Stable, full outer electron shells, rarely undergo chemical reactions.

Ionization and Ionic Character

Ion: Charged atom or group of atoms.
Ionization: Process resulting in ion formation.
Cation: Positively charged ion.
Anion: Negatively charged ion.

Atomic and Ionic Properties

Atomic Radii: Half the distance between nuclei of bonded atoms.
Ionic Radii: Half the diameter of an ion; important in crystal lattice calculations.
Ionization Energy: Energy needed to remove an electron from a neutral atom.
Electron Affinity: Energy change when an electron is gained by a neutral atom.
Electronegativity: Measure of an atom’s ability to attract electrons in a compound.

Pioneers in Chemistry

Stanislao Cannizzaro: Developed methods for accurate atomic mass measurements, aiding standardization.
Dmitri Mendeleev: Created the first Periodic Table, predicting properties of undiscovered elements based on atomic mass.
Henry Moseley: Established the modern Periodic Law, arranging elements by increasing atomic number instead of mass.

Valence Electrons

Group configurations indicate the number of valence electrons: Groups 1 and 2 equal their group number; Groups 13-18 have valence equal to group number minus 10.

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Description

Prepare for your chemistry exam with this study guide focused on Chapter 5. Explore key terms such as periodic law and the periodic table, along with their definitions. Enhance your understanding of how elements are organized and their properties.