Periodic Table Overview
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Questions and Answers

Which of the following elements is classified as a semimetal?

  • Sodium
  • Silicon (correct)
  • Aluminum
  • Calcium

What is the family name of Group 1 elements?

  • Alkali Metals (correct)
  • Alkaline Earth Metals
  • Transition Metals
  • Noble Gases

How many valence electrons do Alkaline Earth Metals have?

  • 4
  • 3
  • 2 (correct)
  • 1

What do members of the same group in the periodic table have in common?

<p>Same number of valence electrons (A)</p> Signup and view all the answers

Why must alkali metals be stored in oil?

<p>To prevent water reactions (C)</p> Signup and view all the answers

What was Mendeleev's main criterion for arranging the original Periodic Table?

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

Which statement accurately describes the arrangement of the modern Periodic Table?

<p>Arranged by atomic number (D)</p> Signup and view all the answers

Which of the following groups contains only nonmetals?

<p>Helium, Nitrogen, Chlorine (B)</p> Signup and view all the answers

What type of ions do nonmetals typically form?

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

Which of the following is NOT a property of metals?

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

How does the metallic character change as you move from left to right across a period?

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

What is the main reason metals generally have low ionization energy?

<p>They do not want to gain electrons (A)</p> Signup and view all the answers

What is the only liquid metal at room temperature?

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

Which trend is observed as you move down a group in relation to ionization energy?

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

Which statement about the states of matter among nonmetals is accurate?

<p>Nonmetals can be solids, liquids, or gases (D)</p> Signup and view all the answers

Which of the following statements is true about nonmetals as you move across a period?

<p>Nonmetallic character increases (A)</p> Signup and view all the answers

What characteristic of metals contributes to their high conductivity?

<p>Freely moving electrons (A)</p> Signup and view all the answers

Which of the following elements is likely to have the highest ionization energy?

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

What is the reason that elements in Group 12 can have multiple positive oxidation states?

<p>They can lose valence electrons from s and/or d orbitals. (C)</p> Signup and view all the answers

Which of the following halogens is a gas at room temperature?

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

Why are noble gases considered inert?

<p>They have full valence shells. (A)</p> Signup and view all the answers

Which element is considered the most active nonmetal?

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

What do electron dot diagrams represent in relation to an atom?

<p>The valence electrons of the atom. (D)</p> Signup and view all the answers

Which of the following statements about the most active metal is true?

<p>It is located in the lower left corner of the table. (A)</p> Signup and view all the answers

What does the kernel represent in an electron dot diagram?

<p>The entire atom excluding the valence electrons. (B)</p> Signup and view all the answers

What is the main difference between a sodium atom and a sodium ion?

<p>The sodium ion has one less energy level than the sodium atom. (A)</p> Signup and view all the answers

Which of the following correctly describes the electron dot diagram for a chloride ion?

<p>8 dots and charge written outside the brackets. (C)</p> Signup and view all the answers

How does the ionic radius of a nonmetal typically compare to its atomic radius?

<p>It is larger because the nonmetal gains electrons. (C)</p> Signup and view all the answers

Which of the following statements is true regarding metals and their ionic forms?

<p>Metals tend to lose their valence electrons. (C)</p> Signup and view all the answers

What do brackets signify in the electron dot diagrams of negative ions?

<p>The acceptance of additional electrons. (A)</p> Signup and view all the answers

What is the charge notation for metallic ions represented in electron dot diagrams?

<p>Charge written to the upper right of the symbol. (A)</p> Signup and view all the answers

What is a common characteristic of the atomic and ionic radius of nonmetals?

<p>Nonmetals have a larger ionic radius than atomic radius. (C)</p> Signup and view all the answers

What happens to the electron configuration when a metal atom forms a positive ion?

<p>Electrons in the outer shell are lost. (B)</p> Signup and view all the answers

What is the primary reason for the significantly higher second ionization energy of sodium compared to its first ionization energy?

<p>The remaining electron is more tightly bound to the nucleus. (D)</p> Signup and view all the answers

Which element has the highest electronegativity based on the content provided?

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

How does electronegativity change as you move down a group in the periodic table?

<p>It decreases. (D)</p> Signup and view all the answers

In ascending order of atomic radius, which of the following sequences is correct?

<p>Mg2+ &lt; Mg &lt; Na &lt; Na+ &lt; Ne &lt; F &lt; O2- (A)</p> Signup and view all the answers

Which factor is primarily responsible for the trend that both ionization energy and electronegativity increase across a period?

<p>Higher nuclear charge with increased protons. (D)</p> Signup and view all the answers

What is the relationship between filling of the outer electron shell and the ionization energy of an atom?

<p>Filled shells generally have higher ionization energy. (A)</p> Signup and view all the answers

Why is the fourth ionization energy of aluminum significantly higher than its third ionization energy?

<p>Aluminum becomes a noble gas configuration after the third ionization. (A)</p> Signup and view all the answers

Which element exhibits the least attraction for electrons based on the electronegativity scale?

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

Flashcards

Atomic number

The modern periodic table is organized by increasing atomic number, which represents the number of protons in an atom.

Metals

Elements located to the left of the stair-step line on the periodic table, except for hydrogen. They tend to lose electrons and form positive ions called cations.

Nonmetals

Elements located to the right of the stair-step line on the periodic table. They tend to gain electrons and form negative ions called anions.

Metalloids

Elements that border the stair-step line on the periodic table. They exhibit properties of both metals and nonmetals.

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Valence Electrons

The number of electrons in the outermost energy level of an atom. It determines the atom's reactivity and bonding behavior.

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Cations

Positively charged ions formed when a metal atom loses electrons.

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Anions

Negatively charged ions formed when a nonmetal atom gains electrons.

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Diatomic Nonmetals

Elements that exist naturally as two atoms bonded together.

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What are semimetals/metalloids?

Elements that share properties of both metals and nonmetals. They can act as semiconductors, meaning they can conduct electricity under certain conditions but not others.

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What are Alkali Metals?

Group 1 on the periodic table, known for their high reactivity with water, forming hydrogen gas and a basic solution.

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What are Valence Electrons?

The number of electrons in the outermost shell of an atom, which determines its reactivity and bonding behavior.

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What are Alkaline Earth Metals?

Group 2 on the periodic table, known for their reactivity, but less than alkali metals. They also exist naturally in compounds.

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What are Transition Metals?

Groups 3-11 on the periodic table, known for their ability to produce color when dissolved in water, due to their constant electron transitions. They are also known to exist in multiple oxidation states.

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Metallic character

Metallic character describes an element's tendency to lose electrons and form positive ions (cations).

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Nonmetallic character

Nonmetallic character describes an element's tendency to gain electrons and form negative ions (anions).

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Ionization energy

Ionization energy (IE) is the minimum energy needed to remove one electron from an atom in its gaseous state, forming a cation.

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Ionization energy trend across a period

Across a period (left to right) on the periodic table, ionization energy generally increases due to increasing nuclear charge and a decreasing atomic radius. However, there are slight variations between s and p sublevel filling.

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Ionization energy trend down a group

Down a group (top to bottom) on the periodic table, ionization energy decreases due to the increasing atomic radius and weaker nuclear attraction to the outermost electrons.

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Halogens

These elements are highly reactive and naturally exist only in compounds.

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Noble gases

These elements are generally unreactive because they have a full outer shell of electrons.

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Most reactive metals

Elements in the lower left corner of the periodic table are the most reactive metals.

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Most reactive nonmetals

Elements in the upper right corner of the periodic table are the most reactive nonmetals.

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Periods on the Periodic Table

The number of occupied electron shells in an atom.

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Groups on the Periodic Table

Elements organized in columns or groups on the periodic table.

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Electron Dot Diagram

A representation of an atom that shows its valence electrons as dots around the element's symbol.

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Atomic Radius

The distance between the nucleus of an atom and its outermost electron shell.

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Ionic Radius

The distance between the nucleus of an ion and its outermost electron shell.

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Ionic Radii vs Atomic radii

Metals tend to lose valence electrons and become smaller, while nonmetals tend to gain electrons and become larger.

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Oxidation Number

The number of electrons an atom must gain or lose to achieve a stable electron configuration (usually 8 valence electrons).

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Ionization

The process of an atom losing or gaining electrons to form a charged particle (ion).

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What is Ionization Energy (IE)?

The minimum amount of energy required to remove one electron from a neutral atom in its gaseous state, forming a positively charged ion (cation).

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Why is the 2nd IE so much higher than the 1st IE?

The energy needed to remove a second electron from an atom that has already lost one electron is significantly higher than the first ionization energy. This is due to the increased positive charge in the remaining ion, which holds the remaining electrons more strongly.

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What factors influence Ionization Energy?

The energy needed to remove an electron from an atom is influenced by factors like atomic radius, nuclear charge, and electron shielding. The higher the nuclear charge or the smaller the atomic radius, the stronger the attraction between the nucleus and the electrons, resulting in higher ionization energy.

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What is Electronegativity?

Electronegativity is a measure of an atom's tendency to attract electrons towards itself when it is part of a chemical bond. It reflects an atom's ability to gain electrons and become negatively charged.

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How does electronegativity change across the periodic table?

Across a period (moving left to right) on the periodic table, electronegativity generally increases. This is because the number of protons increases, leading to a stronger attraction for electrons. Moving down a group (top to bottom), electronegativity generally decreases as the atomic radius increases, weakening the attractive force of the nucleus.

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What is the relationship between Electronegativity and Ionization Energy?

Elements with high electronegativity have a strong tendency to attract electrons, making it difficult to remove them. This means their ionization energy will be high.

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How does atomic radius affect Ionization Energy?

The size of an atom is known as its atomic radius. The larger the radius, the further the valence (outermost) electrons are from the nucleus, and the weaker the attraction between them. As a result, the ionization energy decreases.

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What are Cations and how do they form?

Atoms of the same element can have different numbers of electrons, creating ions with different charges. When an atom loses one or more electrons, it becomes a positively charged ion (cation). Removing another electron from the atom creates a cation with a higher positive charge.

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Study Notes

Periodic Table History

  • Mendeleev arranged the periodic table by atomic mass.
  • Moseley arranged the modern periodic table by increasing atomic number.
  • Reminder: Atomic number is the number of protons.

Basic Periodic Table Setup

  • Metals are to the left of the "step" (staircase) on the table.
  • Nonmetals are to the right of the "step".
  • Metalloids/Semimetals border the "step".

Properties of Metals

  • Metals make up more than half of the elements.
  • Metals are located to the left of the step.
  • Hydrogen is not considered a metal.
  • Metals have relatively low numbers of valence electrons (1-3).
  • Metals tend to lose electrons, forming positive ions (cations).
  • Most metals are solids at room temperature, except for mercury (Hg).
  • Metals are good conductors of heat and electricity due to free-moving electrons.
  • Metals are malleable, ductile, and have high melting points and luster.

Properties of Nonmetals

  • Nonmetals are located to the right of the step.
  • Nonmetals have relatively high numbers of valence electrons (5-8).
  • Nonmetals tend to gain electrons, forming negative ions (anions).
  • Nonmetals can bond with other nonmetals.
  • Nonmetals are poor conductors, good insulators.
  • Nonmetals exist as solids, liquids, or gases. - Hydrogen is a gas - Bromine is a liquid

Properties of Metalloids/Semimetals

  • Metalloids have properties of both metals and nonmetals.
  • Metalloids should be identified by name and symbol.
    • Boron (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te)
  • Aluminum is a metal, not a metalloid.

Groups in the Periodic Table

  • Groups are columns (1-18).

  • Elements in the same group exhibit similar properties due to similar numbers of valence electrons.

  • Alkali Metals are group 1 (IA) metals. -Highly reactive, only found in compounds

    • Naturally only found in compounds
    • One valence electron

  • Alkaline Earth Metals are in group 2 (IIA) -Moderately reactive, exist naturally in compounds -Two valence electrons

  • Transition Metals are groups 3-12 -Various properties, multiple positive oxidation states, produce various colors when dissolved in water.

  • Group 17 (VII A) is called Halogens.

    • Highly reactive, often exist as compounds. -Seven valence electrons -Gain one electron to become a -1 anion.

  • Group 18 (VIII A or 0) is called Noble Gases. -Don't react readily due to filled valence shells.

Finding the Most Reactive Elements

  • Most reactive metal is in the bottom left corner (Francium).
  • Most reactive nonmetal is in the top right corner (Fluorine).

Periods in the Periodic Table

  • Periods are rows (1-7).
  • Properties of elements change across a period.
  • The number of occupied electron shells (principal energy levels) increases across a period.
  • Atoms possess a higher nuclear charge as you move right across a period.

Electron Dot Diagrams/Lewis Dot Diagrams

  • One part of the diagram, the kernel, represents everything that isn't the valence electrons.
  • The other part are dots that represent valence electrons.

Ionization Energy

  • Ionization energy is the energy needed to remove the most loosely held electron from an atom.
  • Metals have low ionization energies; nonmetals have high ionization energies.
  • Ionization energy generally increases going across a row (left to right).
  • Ionization energy generally decreases going down a column (top to bottom).

Electronegativity

  • Electronegativity is an atom's ability to attract and hold electrons when bonded to another atom.
  • Electronegativity generally increases from left to right across a row.
  • Electronegativity generally decreases going down a column.

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Honors Chemistry – Periodic Table PDF

Description

This quiz covers the history and organization of the periodic table, focusing on Mendeleev and Moseley's contributions. You'll learn about the properties of metals and nonmetals, including their positions on the periodic table and characteristics. Test your knowledge on the fundamental aspects of the table's setup.

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