Questions and Answers
Who is known as the Father of the Periodic Table?
Who developed the Modern Periodic Table?
The Periodic Law states that elements are arranged by atomic mass.
False
Define Groups in the periodic table.
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What is the name of Group 1 elements?
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What is the name of Group 2 elements?
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What do you call the elements in Groups 3-11?
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What are the elements in Group 17 called?
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What is the name of the elements in Group 18?
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Define Periods in the periodic table.
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Where are Metals located in the periodic table?
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Where are Non-Metals located in the periodic table?
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What is Ionization Energy?
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What are Metalloids?
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What gases are found on the periodic table?
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Diatomic elements come in pairs.
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Which elements are classified as Liquid Elements?
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What elements are classified as Solid Elements?
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Define Electronegativity.
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How does electronegativity change down a group?
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How does electronegativity change across a period from left to right?
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Which element has the highest electronegativity?
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How does ionization energy change down a group?
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How does ionization energy change across a period?
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What is the definition of atomic radius?
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How does atomic radius change down a group?
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How does atomic radius change across a period from left to right?
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Define Conservation of Energy.
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Define Solubility.
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Study Notes
Father of the Periodic Table
- Mendeleev is recognized as the father of the periodic table for his pioneering work in organizing elements.
Modern Periodic Table
- The modern periodic table was developed by Mosley, focusing on atomic numbers.
Periodic Law
- Elements are arranged by increasing atomic number.
- Elements in the same group exhibit similar chemical properties.
Groups
- Vertical columns in the periodic table.
- Elements within a group react similarly due to having the same number of valence electrons.
- Groups may contain a different number of principal energy levels (PEL).
Alkali Metals
- Group 1 elements are known as alkali metals.
Alkaline Earth Metals
- Group 2 elements are referred to as alkaline earth metals.
Transition Elements
- Groups 3 to 11 are categorized as transition elements.
Halogens
- Group 17 elements are identified as halogens.
Noble Gases
- Group 18 consists of noble gases, characterized by having a complete set of 8 valence electrons.
Periods
- Horizontal rows in the periodic table, with a total of 7 periods.
- Each period represents a different number of electrons, with the same number of PELs.
Metals
- Found to the left of the staircase line on the periodic table.
- Metals have low ionization energy and tend to lose electrons, forming positive ions.
- Excellent conductors of heat and electricity.
Non-Metals
- Located to the right of the staircase.
- Non-metals possess high ionization energy and electronegativity, making them poor conductors of heat and electricity.
- Generally brittle and may shatter.
Ionization Energy
- Defined as the energy required to remove an electron from an atom.
- Having more valence electrons makes it increasingly difficult to remove an electron.
- Noble gases in group 18 (with 8 valence electrons) resist losing electrons.
Metalloids
- Elements that border the staircase, displaying properties of both metals and non-metals.
- Notable metalloids include Boron (B), Silicon (Si), Arsenic (As), Tellurium (Te), Germanium (Ge), and Antimony (Sb).
Gases on the Periodic Table
- Hydrogen (H), Nitrogen (N), Oxygen (O), and Fluorine (F) are diatomic gases, along with the noble gases in group 18.
Diatomic Elements
- Certain elements exist as diatomic molecules, pairing with themselves: H, N, O, and F.
Liquid Elements
- Bromine (Br) and Mercury (Hg) are the only elements that are liquid at room temperature.
Solid Elements
- All other elements that are not classified as liquids or gases, including metalloids.
Electronegativity
- Describes an element's tendency to attract electrons in a chemical bond.
Electronegativity Trends
- Electronegativity decreases down a group as the atomic size increases.
- Electronegativity increases across a period from left to right due to higher nuclear charge.
Highest Electronegativity
- Fluorine (F) possesses the highest electronegativity value of 4.0.
Ionization Energy Trends
- Ionization energy decreases down a group due to increased atomic size.
- Ionization energy increases across a period from left to right as nuclear charge increases.
Atomic Radius
- Defined as half the distance between adjacent nuclei of two atoms.
Atomic Radius Trends
- The atomic radius increases down a group as additional principal energy levels (PEL) are added.
- The atomic radius decreases across a period from left to right due to the increased nuclear charge pulling electrons closer.
Conservation of Energy
- Energy cannot be created or destroyed; it merely transforms from one form to another.
Solubility
- The ability of a substance to dissolve in water, indicating its interactions at the molecular level.
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Description
Test your knowledge of the periodic table with these flashcards focusing on key terms and concepts from the chapter. Learn about Mendeleev's contributions, the modern periodic table, and the periodic law, including the arrangement of elements. Perfect for reinforcing your understanding of the essential elements of chemistry.