Chemistry: Periodic Table and Trends
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Questions and Answers

What charge do transition metals typically acquire when they lose their s2 electron?

  • -2
  • +2 (correct)
  • +1
  • -1

Which group of elements is known for being the most reactive nonmetals?

  • 6
  • 8
  • 1
  • 7 (correct)

Which of the following elements is classified as a lanthanide?

  • 88
  • 106
  • 57 (correct)
  • 90

What is the primary characteristic of noble gases?

<p>They have filled s and p sublevels. (B)</p> Signup and view all the answers

What is the outer electron configuration of the chalcogens?

<p>s2p4 (A)</p> Signup and view all the answers

Which series includes elements that are all radioactive?

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

What is the unique characteristic of hydrogen among the elements?

<p>It has an electron configuration of 1s1. (A)</p> Signup and view all the answers

What is the electron configuration characteristic of elements that become ions with a -1 charge after gaining electrons?

<p>s2p5 (B)</p> Signup and view all the answers

What did Dmitri Mendeleev use to organize the elements in his periodic table?

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

Which element classification is characterized as being soft metals with an s1 electron configuration?

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

What is the primary reason Mendeleev's periodic table displayed irregularities?

<p>He arranged elements by atomic mass. (A)</p> Signup and view all the answers

What discovery did Henry Moseley make regarding elements?

<p>Each element has a unique nuclear charge equivalent to atomic number. (B)</p> Signup and view all the answers

Which group of elements is known for being nonreactive and monoatomic?

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

Elements in the same vertical column of the periodic table are known as what?

<p>Families or groups (C)</p> Signup and view all the answers

What characteristic is specific to alkaline earth metals?

<p>They have an s2 electron configuration. (A)</p> Signup and view all the answers

Which is NOT a property of metals as described in the periodic table?

<p>Brittle when solid (D)</p> Signup and view all the answers

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

<p>More energy levels are being filled with electrons (B)</p> Signup and view all the answers

Which trend describes how ionization energy changes in a group as you move from top to bottom?

<p>Ionization energy decreases (A)</p> Signup and view all the answers

How is the atomic radius of an atom estimated?

<p>By measuring the distance between nuclei and dividing by 2 (C)</p> Signup and view all the answers

Why does electron affinity decrease as you move down a group?

<p>The atoms become larger and the nucleus is further from outer electrons (D)</p> Signup and view all the answers

What is the primary reason atomic radius decreases from left to right across a period?

<p>Increased positive charge of the nucleus draws electrons closer (D)</p> Signup and view all the answers

What happens to the atomic radius when an atom gains an electron?

<p>The atomic radius increases (B)</p> Signup and view all the answers

Which statement accurately describes the trend of ionization energy across a period?

<p>It tends to increase as you move towards noble gases (D)</p> Signup and view all the answers

What effect do inner electrons have on the outer electrons of an atom?

<p>They shield outer electrons from the positive charge of the nucleus (D)</p> Signup and view all the answers

Flashcards

Periodic Table Organization

Elements are arranged in vertical columns (groups) by similar properties and horizontal rows (periods) by increasing atomic mass or atomic number.

Periodic Law

Physical and chemical properties of elements are periodic functions of their atomic number.

Groups (Families)

Elements in the same vertical column of the periodic table; have similar chemical properties and the same valence electron configuration.

Periods

Elements in the same horizontal row of the periodic table; have the same major energy level.

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Alkali Metals

Group 1 elements in the periodic table; soft, highly reactive metals with an s1 valence electron configuration.

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Alkaline Earth Metals

Group 2 elements in the periodic table; relatively reactive metals with an s2 valence electron configuration.

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Atomic Number

The number of protons in the nucleus of an atom.

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Valence Electrons

Electrons in the outermost shell of an atom, determining chemical behavior.

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Atomic Radius Trend (Groups)

Atomic radius increases as you move down a group (column) in the periodic table because electrons occupy higher energy levels, farther from the nucleus.

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Atomic Radius Trend (Periods)

Atomic radius decreases as you move across a period (row) in the periodic table because the increasing nuclear charge pulls the electrons closer to the nucleus.

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Ionization Energy Trend (Groups)

Ionization energy decreases as you move down a group (column) due to shielding, where inner electrons block the outer electrons from the nucleus's attraction.

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Ionization Energy Trend (Periods)

Ionization energy generally increases as you move across a period (row) due to the increasing nuclear charge.

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Electron Affinity Trend (Groups)

Electron affinity generally decreases as you move down a group (column) because larger atoms have outer electrons farther from the nucleus, making it less attractive to gain another electron.

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Electron Affinity Trend (Periods)

Electron affinity generally increases as you move across a period (row) because atoms are closer to achieving a full electron shell, making them more eager to gain electrons.

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What is atomic radius?

The distance between the nucleus of an atom and its outermost electron shell, giving an idea of the atom's size.

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What is ionization energy?

The amount of energy needed to remove one electron from a neutral atom in its gaseous state.

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Transition Metals

Elements in Groups 3 through 12 of the periodic table, known for their hardness, less reactivity compared to Groups 1 and 2, and filling of the d-orbital in their outer shells.

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Lanthanides

The series of elements with atomic numbers 57-71, known for their shine, reactivity, and use as phosphors that glow when struck by electrons.

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Actinides

The series of elements with atomic numbers 89-103, known for being radioactive, with many being man-made. Uranium is a significant element in nuclear energy reactions.

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Main Block Elements

Elements in Groups 3 through 8 of the periodic table, encompassing metals like aluminum and lead, metalloids like silicon, and nonmetals like oxygen and chlorine.

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Halogens

Group 7 elements, known for their high reactivity as nonmetals, forming salts with Group 1 metals. They gain one electron to achieve the electron configuration of a noble gas.

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Chalcogens

Group 6 elements, known for gaining two electrons to achieve the electron configuration of a noble gas, forming -2 charged ions. Oxygen is the most reactive element in this group.

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Noble Gases

Group 8 elements, characterized by a full s and p sublevel in their highest energy level, making them stable and unreactive.

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Hydrogen

An element with unique properties, existing on its own in the periodic table. It can act as a metal or nonmetal, typically sharing its electron and reacting with other molecules.

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Study Notes

Transition Metals and Charge

  • Transition metals typically acquire a +2 charge when they lose their s2 electrons.

Most Reactive Nonmetals

  • The halogens are known for being the most reactive nonmetals.

Lanthanide Element

  • Cerium (Ce) is classified as a lanthanide.

Noble Gases Characteristic

  • Noble gases are characterized by their lack of reactivity due to their full outer electron shells.

Chalcogens Outer Electron Configuration

  • Chalcogens have an outer electron configuration of ns2np4.

Radioactive Elements

  • All elements in the actinide series are radioactive.

Hydrogen's Uniqueness

  • Hydrogen is unique among the elements because it is the only element that can exist as both a metal and a nonmetal.

-1 Charge Ion Configuration

  • Elements with an outer electron configuration of ns2np5 gain one electron to achieve a stable octet configuration, becoming ions with a -1 charge.

Mendeleev's Periodic Table Organization

  • Dmitri Mendeleev organized the elements in his periodic table by atomic weight.

Soft Metals with s1 Configuration

  • Alkali metals are characterized as soft metals with an s1 electron configuration.

Mendeleev's Periodic Table Irregularities

  • Mendeleev's periodic table displayed irregularities because he relied on atomic weight rather than atomic number.

Moseley's Discovery Regarding Elements

  • Henry Moseley discovered that the atomic number, not atomic weight, is the fundamental property that determines an element's chemical behavior.

Nonreactive and Monoatomic Elements

  • Noble gases are known for being nonreactive and monoatomic.

Elements in Same Vertical Column

  • Elements in the same vertical column of the periodic table are called a group.

Alkaline Earth Metal Characteristic

  • Alkaline earth metals are characterized by having two electrons in their outermost shell.

Metal Properties

  • Brittleness is NOT a typical property of metals as described in the periodic table.

Atomic Radius Increase Down a Group

  • The atomic radius increases as you move down a group due to the addition of electron shells.

Ionization Energy Trend Down a Group

  • Ionization energy decreases as you move down a group because the outermost electrons are farther from the nucleus and easier to remove.

Atomic Radius Estimation

  • The atomic radius of an atom is estimated by measuring the distance between the nuclei of two identical atoms bonded together.

Electron Affinity Decrease Down a Group

  • Electron affinity decreases as you move down a group because the outer electrons are farther from the nucleus and less attracted to the nucleus.

Atomic Radius Decrease Across a Period

  • The atomic radius decreases from left to right across a period because the number of protons in the nucleus increases, increasing the attraction between the nucleus and electrons, pulling them closer.

Atomic Radius Change with Electron Gain

  • When an atom gains an electron, its atomic radius increases because the added electron increases the electron-electron repulsion, pushing the electrons farther apart.

Ionization Energy Trend Across a Period

  • Ionization energy increases across a period because the increasing nuclear charge attracts the electrons more strongly, making them harder to remove.

Inner Electrons Effect on Outer Electrons

  • Inner electrons shield the outer electrons from the full nuclear charge, reducing the attraction between the nucleus and the outer electrons.

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Related Documents

Periodic Trends PDF

Description

Explore the fascinating history and development of the periodic table, from Mendeleev's initial arrangements to Moseley's corrections based on atomic number. Discover how electron configurations define element placement and properties within the table. This quiz covers key concepts and participants in the evolution of chemical organization.

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