Chemistry Periodic Table Quiz

Periodic Table

• The periodic table organizes elements in a specific way.
• A significant amount of information about an element can be obtained from its position in the table.
• Predicting physical and chemical properties of an element is possible using the periodic table.
• The periodic table helps understand how elements react with other elements.
• The table contains basic information on all 118 known elements.

Learning Objectives

• Understand why chemists use the periodic table.
• Identify the location of groups, periods, and transition metals within the table.
• Analyze periodic trends in ionization energy, atomic radius, and electronegativity.
• Connect periodic trends to the atomic structure of elements.

Periodic Law

• The repeating physical and chemical properties of elements change periodically with the atomic number.

What's in a Square?

• Each element square contains unique information, like:
  • Symbol
  • Average atomic mass
  • Physical state (gas, liquid, solid)
  • Atomic number
  • Name
  • Valence electrons

Hydrogen

• Hydrogen sits above Group Al, but it's a unique element.
• Hydrogen is a gas at room temperature.
• It has one proton and one electron in its single energy level.
• It needs 2 electrons to fill its valence shell.

Atomic Mass Unit (AMU)

• The unit for measuring an atom's mass is the AMU.
• AMU stands for atomic mass unit.
• One AMU equals the mass of one proton.
• There are 6.02 x 10^23 AMUs in one gram.
• Electrons are much smaller than one AMU.

Symbols

• Each element has its own unique symbol.
• A symbol can be one capital letter or a capital letter followed by one or two lowercase letters.
• Examples include carbon (C) and copper (Cu).

Common Elements and Symbols

• A table is provided listing various elements and their symbols.

Classification of Elements in the Periodic Table

• Elements are categorized into groups (vertical columns) and periods (horizontal rows).

Properties of Metals

• Metals are good conductors of heat and electricity.
• Metals are typically shiny.
• Metals can be drawn into wires (ductile) and hammered into sheets (malleable).
• A chemical property of metals is their reaction with water, which can result in corrosion.

Properties of Metalloids

• Metalloids have properties of both metals and nonmetals.
• Metalloids are usually solid.
• Metalloids can be shiny or dull.
• Metalloids are better electrical conductors than nonmetals but not as good as metals.
• Metalloids are ductile and malleable.

Properties of Nonmetals

• Nonmetals are poor conductors of heat and electricity.
• Solid nonmetals are usually brittle and break easily.
• Nonmetals are typically dull.
• Many nonmetals are gases.

Rare Earth Elements

• Thirty rare earth elements are composed of lanthanide and actinide series.
• Most lanthanide series and transuranium/actinide elements are synthetic substances.

Mendeleev

• Dmitri Mendeleev created the first accepted periodic table in 1869.
• It grouped elements according to atomic mass and similar chemical properties.
• This table included blank spaces to accommodate future discoveries of elements.

Matter

• All matter consists of atoms and atom groups bonded together, called molecules. Pure substances are made of only one type of atom. Substances made from more than one type of atom form compounds. Mixtures result from combining compounds physically without chemical bonding.

Elements, Compounds, Mixtures

• Sodium and chlorine combine chemically to form sodium chloride, commonly known as table salt, a compound.
• Elements, compounds, and mixtures can be separated by different methods.
• Mixtures separate using physical methods whereas compounds need chemical methods to separate.
• Elements are pure substances.

Trends in the Periodic Table

• Trends in the periodic table are predictable changes in various properties.
• Atomic number affects nuclear attraction across a period (increasing attraction).
• Shielding effect causes decrease in nuclear attraction down a group.

Atomic Radius

• Atomic radius is the distance from an atom's center to its outermost electrons.

Atomic Radius Trend

• The atomic radius generally increases down a group and decreases across a period.

Ionization Energy Trend

• Ionization energy is the energy needed to remove an electron from an atom or ion.
• Ionization energy generally increases across a period and decreases down a group.

Electronegativity Trend

• Electronegativity is an atom's ability to attract electrons in a chemical bond.
• Electronegativity generally increases across a period.
• Electronegativity generally decreases down a group.

What is a Compound?

• A compound is a substance formed when two or more different elements are chemically bonded.

What is the chemical bond?

• The question provides an inquiry, not a statement.

Reference

• Information was sourced from various general chemistry, organic chemistry, biochemistry texts and the internet.

Test your understanding of the periodic table with this quiz. Explore how elements are organized and learn about periodic trends, groups, and transitions. Gain insight into the unique information contained within each element square.