Periodic Table Classification
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Questions and Answers

Who first published the classification of the elements that is the basis of our periodic table today?

Dmitri Mendeleev

By what property did Mendeleev arrange the elements?

Atomic Mass

By what property did Moseley suggest that the periodic table be arranged?

Atomic Number

What is the periodic law?

<p>The properties of the elements repeat periodically.</p> Signup and view all the answers

What is a period in the periodic table? How many are there?

<p>A horizontal row in the periodic table. There are seven periods.</p> Signup and view all the answers

What is a group (also called a family)? How many are there in the periodic table?

<p>A vertical column in the periodic table. There are 18 groups.</p> Signup and view all the answers

State the number of valence electrons in an atom of sulfur.

<p>6</p> Signup and view all the answers

State the number of valence electrons in an atom of calcium.

<p>2</p> Signup and view all the answers

State the number of valence electrons in an atom of chlorine.

<p>7</p> Signup and view all the answers

State the number of valence electrons in an atom of arsenic.

<p>5</p> Signup and view all the answers

What element corresponds to the atomic number 10?

<p>Ne; Neon</p> Signup and view all the answers

What element corresponds to the atomic number 18?

<p>Ar; Argon</p> Signup and view all the answers

List, by number, both the period and group of the element beryllium.

<p>Be 2 2</p> Signup and view all the answers

What element corresponds to the atomic number 36?

<p>Kr; Krypton</p> Signup and view all the answers

What element corresponds to the atomic number 90?

<p>Th; Thorium</p> Signup and view all the answers

List, by number, both the period and group of the element iron.

<p>Fe 4 8</p> Signup and view all the answers

List, by number, both the period and group of the element lead.

<p>Pb 6 14</p> Signup and view all the answers

How does an element's period number relate to the number of the energy level of its valence electrons?

<p>Period Number = Energy level of valence electrons</p> Signup and view all the answers

What are the transition elements?

<p>They are the D-block elements and are located in Groups 3 through 12.</p> Signup and view all the answers

Would you expect strontium to be chemically more similar to calcium or rubidium and why?

<p>It would be more similar to calcium because strontium and calcium have two valence electrons.</p> Signup and view all the answers

What is the heaviest noble gas?

<p>Radon</p> Signup and view all the answers

What is the heaviest alkaline earth metal?

<p>Radium</p> Signup and view all the answers

In going from top to bottom of any group, each element has ? more occupied energy level(s) than the element above it.

<p>1</p> Signup and view all the answers

What are the Group 1 elements called?

<p>Alkali Metals</p> Signup and view all the answers

What are the Group 2 elements called?

<p>Alkaline Earth Metals</p> Signup and view all the answers

What are the Group 17 elements called?

<p>Halogens</p> Signup and view all the answers

What are the Group 18 elements called?

<p>Noble Gases</p> Signup and view all the answers

What is the name of the elements in Groups 3 to 12?

<p>Transition metals</p> Signup and view all the answers

List the three lightest members of the noble gases.

<p>He, Ne, Ar</p> Signup and view all the answers

List all of the alkali metals.

<p>Li, Na, K, Rb, Cs, Fr</p> Signup and view all the answers

Why do all the members of a group have similar properties?

<p>They have the same number of valence electrons.</p> Signup and view all the answers

What do we mean by the 'atomic radius'?

<p>The size of a neutral (not ionic) atom.</p> Signup and view all the answers

Within a group, what happens to the atomic radius as you go down the column?

<p>Increases</p> Signup and view all the answers

Why does the atomic radius change?

<p>The addition of one energy level as you move down the group.</p> Signup and view all the answers

Within a period, what happens to the atomic radius as the atomic number increases?

<p>Decreases</p> Signup and view all the answers

Why does the atomic radius change?

<p>No additional energy levels are added; however, more protons are added (increased nuclear charge) to the nucleus increasing the pull on the electrons.</p> Signup and view all the answers

How are neutral atoms converted into cations?

<p>Loss of electrons</p> Signup and view all the answers

How are neutral atoms converted into anions?

<p>Gain of electrons</p> Signup and view all the answers

Metals usually form what type of ions?

<p>Cations (positive)</p> Signup and view all the answers

Nonmetals usually form what type of ions?

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

What is ionization energy?

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

What is the general trend of ionization energy as you go from left to right across the periodic table?

<p>Increases due to increased nuclear charge (protons hold onto the electrons tightly)</p> Signup and view all the answers

What is the general trend of ionization energy as you go down a group on the periodic table?

<p>Decreases due to the larger size of the atom and electrons shielding; both reduce the pull of the nucleus on the electrons.</p> Signup and view all the answers

Which of these elements has the highest first ionization energy: Sn, As, or S?

<p>S</p> Signup and view all the answers

Where, generally, are the metals located on the periodic table?

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

Where, generally, are the nonmetals located on the periodic table?

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

List some properties of metals.

<p>Lose electrons to form positive ions (cations); good conductors of heat and electricity; malleable (able to be hammered into sheets); ductile (can be pulled into wires); have luster (shiny); solid at room temperature except for mercury.</p> Signup and view all the answers

List some properties of nonmetals.

<p>Gain electrons to form negative ions (anions); poor conductors of heat and electricity; brittle (not malleable or ductile); dull (not shiny); some are solid, some are liquid and some are gas at room temperature.</p> Signup and view all the answers

What kinds of properties do metalloids have?

<p>Properties of both metals and nonmetals.</p> Signup and view all the answers

What is electronegativity?

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

What is the general trend of electronegativity as you go down the periodic table?

<p>Decreases due to added energy levels and electron shielding which reduces the pull of the nucleus on the electrons.</p> Signup and view all the answers

What is the general trend of electronegativity as you go left to right across the periodic table?

<p>Increases due to the additional nuclear charge (protons) while NOT adding any energy levels.</p> Signup and view all the answers

Study Notes

Periodic Table Classification

  • Dmitri Mendeleev published the first classification of elements.
  • Mendeleev arranged the periodic table by atomic mass.
  • Moseley suggested arranging elements by atomic number.

Periodic Law and Structure

  • Periodic law states that element properties repeat periodically.
  • A period refers to a horizontal row; there are seven periods in the periodic table.
  • A group (or family) is a vertical column; there are 18 groups.

Valence Electrons

  • Sulfur has 6 valence electrons.
  • Calcium has 2 valence electrons.
  • Chlorine has 7 valence electrons.
  • Arsenic has 5 valence electrons.

Element Identification

  • Neon (Ne) is the element with atomic number 10.
  • Argon (Ar) is the element with atomic number 18.
  • Beryllium (Be) is in period 2, group 2.
  • Krypton (Kr) has atomic number 36.
  • Thorium (Th) has atomic number 90.
  • Iron (Fe) is located in period 4, group 8.
  • Lead (Pb) is located in period 6, group 14.

Energy Levels and Valence Electrons

  • An element's period number corresponds to its valence electrons' energy level.
  • Transition elements are D-block elements located in groups 3 through 12.
  • Group 1 elements are known as alkali metals; Group 2 elements are alkaline earth metals.
  • Group 17 elements are called halogens, while Group 18 elements are noble gases.
  • Elements in groups 3 to 12 are referred to as transition metals.

Noble Gases and Alkali Metals

  • The three lightest noble gases are Helium (He), Neon (Ne), and Argon (Ar).
  • Alkali metals include Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), and Francium (Fr).
  • Atomic radius is defined as the size of a neutral atom.
  • Within a group, the atomic radius increases as you move down the column.
  • Atomic radius decreases across a period with increasing atomic number due to added protons.

Ion Formation

  • Neutral atoms can become cations (positive ions) through electron loss.
  • Neutral atoms can become anions (negative ions) through electron gain.
  • Metals typically form cations, while nonmetals form anions.

Ionization Energy

  • Ionization energy is the energy needed to remove an electron from an atom.
  • Ionization energy generally increases from left to right across the periodic table due to increased nuclear charge.
  • Ionization energy decreases down a group because of increased atomic size and electron shielding.

Element Locations

  • Metals are generally located to the left of the stairstep on the periodic table.
  • Nonmetals are located to the right of the stairstep.

Properties of Metals and Nonmetals

  • Metals lose electrons to form cations, are good conductors of heat and electricity, are malleable and ductile, and are usually solid at room temperature (except mercury).
  • Nonmetals gain electrons to form anions, are poor conductors, are brittle, and can be gas, liquid, or solid at room temperature.

Metalloids and Electronegativity

  • Metalloids exhibit properties of both metals and nonmetals.
  • Electronegativity measures an atom's ability to attract electrons.
  • Electronegativity decreases down the periodic table and increases from left to right due to increased nuclear charge.

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Description

Test your knowledge on the periodic table, including the classification of elements, periodic law, and valence electrons. Understand how to identify elements based on their atomic numbers and positions within the table. This quiz covers key concepts related to chemistry and atomic structure.

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