The Periodic Table - History and Structure
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Questions and Answers

What is the trend in atomic radius as you move down a group in the periodic table?

  • The atomic radius increases. (correct)
  • The atomic radius remains constant.
  • The atomic radius first decreases and then increases.
  • The atomic radius decreases.

What three factors influence periodic trends?

  • Electronegativity, atomic radius, and conductivity.
  • Energy level, charge on nucleus, and shielding effect. (correct)
  • Nuclear charge, electron affinity, and density.
  • Energy level, atomic mass, and ionization energy.

Which type of elements are referred to as inner transition metals?

  • Elements filling the 'f' sublevel. (correct)
  • Elements in Group A.
  • Elements filling the 's' sublevel.
  • Elements located in the top rows of the table.

Why does atomic size decrease as you move across a period from left to right?

<p>More protons increase the nuclear charge. (C)</p> Signup and view all the answers

How are the f orbitals filled in terms of periodic table periods?

<p>They start filling at the 4th period. (D)</p> Signup and view all the answers

What was the primary contribution of J.W. Dobereiner to the development of the periodic table?

<p>Grouping elements into triads based on similar properties (D)</p> Signup and view all the answers

Which scientist is credited with predicting the properties of undiscovered elements?

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

How are groups or families in the periodic table organized?

<p>In vertical columns based on similar properties (A)</p> Signup and view all the answers

Which of the following elements belongs to the noble gases group?

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

What characteristic is common among metals in the periodic table?

<p>They are good conductors of heat and electricity. (A)</p> Signup and view all the answers

Which electron configuration corresponds to the element Potassium (K)?

<p>1s2 2s2 2p6 3s2 3p6 4s1 (D)</p> Signup and view all the answers

Where on the periodic table would you find metalloids?

<p>Along the zig-zag line dividing metals and nonmetals (C)</p> Signup and view all the answers

Which term describes the arrangement of elements based on increasing atomic number?

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

What is true about the elements in group 1A (1)?

<p>They are called Alkali Metals and typically form bases in water. (C)</p> Signup and view all the answers

Which class of elements is primarily associated with being poor conductors and brittle?

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

What is an ion?

<p>An atom with a positive or negative charge (C)</p> Signup and view all the answers

What type of ion is formed when sodium loses an electron?

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

What charge does chlorine acquire when it gains an electron?

<p>-1 (C)</p> Signup and view all the answers

How does ionization energy trend across a period in the periodic table?

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

Which statement correctly describes the second ionization energy compared to the first ionization energy?

<p>It is always greater than the first ionization energy. (D)</p> Signup and view all the answers

What happens to ionization energy as you move down a group in the periodic table?

<p>It decreases due to increased electron shielding. (C)</p> Signup and view all the answers

What is the charge designation for a cation formed by magnesium when it loses two electrons?

<p>Mg2+ (D)</p> Signup and view all the answers

Which element would most likely form a cation?

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

What happens to the first ionization energy (IE) as you move down a group in the periodic table?

<p>IE decreases due to increased distance from the nucleus. (D)</p> Signup and view all the answers

Which of the following correctly states the relationship between nuclear charge and ionization energy?

<p>Higher nuclear charge leads to increased ionization energy. (D)</p> Signup and view all the answers

Which of the following trends is observed in the size of cations across a period from left to right?

<p>Cations get smaller due to increased nuclear charge. (C)</p> Signup and view all the answers

What explains the decrease in ionization energy down a group?

<p>Increased energy levels leading to further distance from nucleus. (B)</p> Signup and view all the answers

Which of the following ions is isoelectronic with Ne?

<p>Mg2+ (B)</p> Signup and view all the answers

How does electron shielding impact ionization energy?

<p>Decreases ionization energy, making it easier to remove the outer electron. (C)</p> Signup and view all the answers

Which statement accurately describes the size of isoelectronic ions?

<p>Positive ions are smaller than negative ions with the same electron count. (B)</p> Signup and view all the answers

Why do noble gases require a significant amount of energy to remove their electrons?

<p>Because they have a full outer energy level. (D)</p> Signup and view all the answers

Which group of elements typically does not react due to having a full outer shell?

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

What characterizes the representative elements in groups 1A through 7A?

<p>Display a wide range of properties (D)</p> Signup and view all the answers

In which columns of the periodic table are transition metals found?

<p>Columns 3B to 12B (D)</p> Signup and view all the answers

What is the state of the d sublevel in transition metals?

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

How are the outer electrons of noble gases configured?

<p>Both s and p sublevels are filled (C)</p> Signup and view all the answers

Which of the following is true of the electron configuration for transition metals?

<p>The d orbitals fill in levels that are one less than the period number (B)</p> Signup and view all the answers

What is the defining characteristic of inner transition metals?

<p>Their f sublevels are filling (A)</p> Signup and view all the answers

Which group ends with an incompletely filled outer s or p sublevel?

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

Flashcards

Periodic Table Arrangement

Elements are arranged by increasing atomic number, showing repeating physical and chemical properties.

Periodic Table - Groups

Vertical columns on the table, also known as families, with elements sharing similar properties due to similar valence electron configuration.

Periodic Table - Periods

Horizontal rows on the table, corresponding to electron energy levels filled in order.

Representative Elements

Elements in groups 1A through 8A, displaying varied properties.

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Alkali Metals

Group 1A elements (excluding hydrogen) reacting strongly with water to form bases.

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Alkaline Earth Metals

Group 2A elements, also reacting with water to form bases, but less reactive than alkali metals.

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Halogens

Group 7A (17) elements, forming salts by reacting with other elements in the table.

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Noble Gases

Group 8A (18) elements, characterized by their unreactivity due to full electron shells.

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Metals

Elements primarily on the left side of the table, good conductors of heat and electricity, often lustrous, ductile, and malleable.

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Electron Configuration

Arrangement of electrons in an element's orbitals, determining that element's properties and position in the Periodic Table.

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Transition Metals

Elements in the 'B' columns of the periodic table. Their 'd' sublevel is filling.

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Noble Gas Configuration

Outer s and p sublevels are completely filled in noble gases.

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d-block

Portion of the periodic table where the 'd' orbitals are filling, containing transition metals.

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Period Numbers

Number representing a horizontal row in the periodic table.

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Sublevels (s, p, d, f)

Within electron orbitals, these specific energy levels hold electrons.

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Atomic Radius Trend (Group)

Atomic radius increases as you move down a group on the periodic table.

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Atomic Radius Trend (Period)

Atomic radius decreases as you move across a period on the periodic table.

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Inner Transition Metals

Located below the main body of the periodic table, filling the 'f' sublevel.

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Periodic Trends Factors

Changes in periodic properties are influenced by energy level, nuclear charge, and shielding.

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Atomic Radius Measurement

Half the distance between the nuclei of two atoms bonded together.

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Ion

An atom (or group of atoms) with a positive or negative charge.

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Cation

A positively charged ion.

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Anion

A negatively charged ion.

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Ionization Energy

The energy needed to remove an electron from a gaseous atom.

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First Ionization Energy

The energy required to remove the first electron from an atom.

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Metals lose electrons

Metals tend to lose electrons in chemical reactions to form positive ions (cations).

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Nonmetals gain electrons

Nonmetals tend to gain electrons in chemical reactions to form negative ions (anions).

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Multiple Ionization Energies

Subsequent energy required to remove additional electrons from an atom after the first has been removed.

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Ionization Energy (IE)

The minimum amount of energy required to remove an electron from a gaseous atom in its ground electronic state to form a cation.

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Factors Affecting IE

Ionization energy is influenced by:

  1. Nuclear Charge: Greater nuclear charge increases attraction, raising IE.
  2. Distance from Nucleus: Greater distance weakens attraction, lowering IE.
  3. Shielding Effect: Inner electrons block the nucleus' attraction, lowering IE on outer electrons.
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IE - Group Trend

Ionization energy decreases as you move down a group on the periodic table. This is because:

  1. Increased distance from nucleus: Electrons are further away, feeling less attraction.
  2. Increased shielding: More inner electrons block the nucleus' attraction.
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IE - Period Trend

Ionization energy generally increases as you move across a period on the periodic table. This is because:

  1. Increased nuclear charge: Stronger nucleus attracts electrons more tightly.
  2. Same shielding: Electrons are in the same energy level, experiencing the same shielding.
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Ion Group Trend

As you move down a group, ions become larger. This is because each step down adds an energy level, increasing size. For example, Li1+, Na1+, K1+, Rb1+, Cs1+.

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Ion Period Trend

Cations (positive ions) become smaller as you move across a period. Anions (negative ions) also get smaller, but are always larger than cations in the same energy level.

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Isoelectronic Ions

Isoelectronic ions have the same number of electrons, but different numbers of protons. For example, Al3+, Mg2+, Na1+, Ne, F1-, O2- and N3- all have 10 electrons.

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Size of Isoelectronic Ions

Isoelectronic ions with more protons are smaller. This is because the stronger nuclear charge pulls the electrons more tightly.

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Study Notes

The Periodic Table - History

  • J.W. Dobereiner (1829): Published a system grouping elements with similar properties into sets of three. The middle element had an atomic weight between the other two. Example elements: Lithium (Li), Sodium (Na), Potassium (K); Calcium (Ca), Strontium (Sr), Barium (Ba).

  • Dmitri Mendeleev (1869): Organized elements by repeating properties based on atomic mass. Left spaces for undiscovered elements and predicted their properties.

  • Henry Moseley (1913): Discovered atomic number and determined the atomic number for known elements of his time. This became the organizing principle for the modern periodic table.

The Periodic Table - Today

  • Arranged by atomic number
  • Periods are rows
  • Groups/Families are columns
  • Elements are in periods based on filling electron shells, which correspond to energy levels
  • Elements in the same group have similar chemical properties because their outermost electrons are the same.

Squares in the Periodic Table

  • Symbols and names of elements
  • Information about their atomic structure (varies by table)
  • Atomic number and atomic mass
  • Color codes: Black = solid, Red = gas, Blue = liquid
  • Electron configurations (sometimes included)

Arrangement - Columns (Groups/Families)

  • Groups/families form vertical columns.
  • Some tables use numerical labels (1-18).
  • Many groups have family names, like:
    • Alkali Metals (Group 1A/1): Reactive metals that form bases in water
    • Alkaline Earth Metals (Group 2A/2): Metals that also form bases but aren't as reactive.
    • Halogens (Group 7A/17): Reactive nonmetals that form salts.
    • Noble Gases (Group 8A/18): Very stable, unreactive nonmetals.

Arrangement - Rows (Periods)

  • Periods form rows (7 rows)
  • The order of filling electron shells determines the period for each element
  • Each period corresponds to an energy level. Elements in the same period have the same outermost energy level

Classes of Elements

  • Metals: On the left side of the table (about 80%). Good conductors of heat and electricity. Solid at room temperature (except mercury). Lustrous (reflect light). Ductile (can be drawn into wires). Malleable (can be hammered into sheets).
  • Nonmetals: On the upper right side of the table. Properties vary greatly. Most are gases, some are solids (e.g., bromine is a liquid). Mostly poor conductors. Brittle.
  • Metalloids: Between metals and nonmetals. Show properties of both. Examples include Boron (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te), and Astatine (At).

Electron Configurations

  • Elements in the same group have the same outermost electron configuration and valence number, explaining their similar properties.
  • The table is organized by blocks, based on the types of orbitals being filled (such as s, p, d, and f).

Elements in the s-block

  • Alkali metals end in s¹
  • Alkaline earth metals end in s² (and He, though placed differently)

Main Groups

  • Based on electron configuration, there are 4 main groups:
    • Noble gases
    • Representative elements
    • Transition metals
    • Inner transition metals.

Electron Configurations in Groups

  • Noble gases (Group 8A/18): Very stable, do not usually react. Outer s and p sublevels are completely filled.
  • Representative elements (Groups 1A through 7A): Display widely varied properties. End with s or p sublevels (but are not always filled completely)
  • Transition metals (Groups 3B through 12B): D-block elements. "Transition" from metal to nonmetal properties; d sublevel is filling.
  • Inner transition metals: F-block elements. Filling the f sublevel and are placed separately in two rows below the main table.

Ionization Energy

  • Energy required to remove an electron from a gaseous atom
  • Increases across a period (left to right) due to increasing nuclear charge.
  • Decreases down a group (top to bottom) due to increasing atomic size and shielding.
  • Multiple ionization energies are greater than the first one

Atomic Radius

  • Distance from the center of the nucleus to the outermost electron.
  • Increases down a group because of new energy levels (electron shells).
  • Decreases across a period due to increasing nuclear charge pulling on the orbitals.

Electronegativity

  • Ability of an atom to attract electrons in a chemical bond.
  • Increases across a period (left to right)
  • Decreases down a group (top to bottom).

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Periodic Table 2016 (PDF)

Description

Explore the fascinating journey of the periodic table from its historical origins to its modern arrangement. Learn about key figures like J.W. Dobereiner, Dmitri Mendeleev, and Henry Moseley, and understand how elements are organized by atomic number, periods, and groups today. This quiz will test your knowledge on the evolution and current structure of the periodic table.

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