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Questions and Answers
Who is known as the 'Father of the Modern Periodic Table'?
The Law of Triads was proposed by Henry G. Moseley.
False
What significant arrangement of elements did Henry G. Moseley develop?
Increasing atomic number
The symbol for Iron is ______.
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Match the following elements with their Latin names:
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Which law states there is a repetition of similar properties for every eighth element?
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Every element's chemical symbol is unique and may be derived from its name.
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What primary concept did Mendeleev's periodic table utilize for arranging elements?
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What property do metalloids exhibit that distinguishes them from metals and non-metals?
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Metals gain electrons to form positively charged ions.
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What is the term for the amount of energy required to remove an electron from an atom?
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Metals are typically considered _______ because they lose electrons to form cations.
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Match the following concepts to their definitions:
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Which of the following elements has the symbol 'Na'?
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Period 6 of the periodic table can have up to 32 elements.
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What family do Group 7A elements belong to?
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The chemical symbol for Tin is ______.
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Match the following groups with their corresponding families:
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Which group of the periodic table contains the transition elements?
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Noble gases exhibit high reactivity.
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How many elements does Period 4 have?
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Which block of elements corresponds to the highest main energy level of the outer electrons?
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Metals are generally located on the right side of the periodic table.
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What element grouping do lanthanide and actinide elements belong to?
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Elements in the same group have similar outer electronic configurations or last sublevel configurations known as _____ configurations.
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Match the following groups with their corresponding characteristics:
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What characteristic do non-metals typically exhibit in reactions with metals?
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Elements with three or fewer electrons in the outer energy level are typically classified as non-metals.
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What is a common property of metals?
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Study Notes
Periodic Table of Elements
- The periodic table is a chart that organizes the chemical elements by atomic number, electron configuration, and recurring chemical properties.
- Johann Dobereiner (1817) developed the Law of Triads. Elements with similar properties were arranged in groups of three. Examples include: Chlorine, Bromine, Iodine; Iron, Cobalt, and Nickel.
- John Newlands (1864) proposed the Law of Octaves. This states that there is a repetition of similar properties for every eighth element. Examples include: Fluorine and Chlorine, lithium and Sodium.
- Julius Lothar Meyer (1869) developed a periodic table with 56 elements, grouped according to their valence and properties.
- Dmitri Mendeleev (1869) is considered the "Father of the Modern Periodic Table". He arranged the elements by increasing atomic weight, grouping elements with similar properties in the same column.
- Henry G. Moseley (1913) determined the atomic number for each element and rearranged the periodic table by increasing atomic number. He proposed the modern periodic law, which states that the chemical and physical properties of elements are a periodic function of their atomic numbers.
- The element symbol is the shorthand for the element. Many symbols are derived from the first letter or two letters of the element's name. Some symbols are derived from their Latin names.
- Antimony - Sb - Stibium
- Copper - Cu - Cuprum
- Gold - Au - Aurum
- Iron - Fe - Ferrum
- Lead - Pb - Plumbum
- Mercury - Hg - Hydragyrum
- Potassium - K - Kalium
- Silver - Ag - Argentum
- Sodium - Na - Natrium
- Tin - Sn - Stannum
- Tungsten - W - Wolfram
Periods and Groups
- Periods are the horizontal rows on the periodic table. There are seven periods.
- Period 1: 2 elements with 2 electrons in the s sublevel.
- Period 2 & 3: 8 elements with 8 electrons in the s and p sublevels.
- Period 4 & 5: 18 elements with 18 electrons in the s, p, and d sublevels.
- Period 6: 32 elements with 32 electrons in the s, p, d, and f sublevels.
- Period 7: Still incomplete but elements fill up s, p, d and f sublevels.
- Groups/Families are vertical columns divided into A and B subgroups.
- A Groups:
- 1A: Alkali metals
- 2A: Alkaline earth metals
- 3A: Boron Family
- 4A: Carbon Family
- 5A: Nitrogen Family
- 6A: Oxygen Family
- 7A: Halogens
- 8A: Noble/Inert Gases
- B Groups: Transition Elements
- A Groups:
Classification of Elements
- Representative elements: These are the elements in columns 1A to 7A. They are characterized by the stepwise addition of electrons to the s and p sublevels.
- Noble or Inert Gases: These are the elements in Group 8A. They have a completely filled set of s and p sublevels. They are colorless and unreactive.
- Transition Elements: These are the elements in columns 1B to 8B. They are characterized by the stepwise addition of electrons to the d sublevel.
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Inner-Transition Elements: These are the two horizontal rows below the main periodic table.
- Lanthanides: The elements after Lanthanum in period 6, all metals. They are also known as Rare Earth elements.
- Actinides: The elements after Actinium in period 7. These are all radioactive and known as heavy Rare Earth elements.
Position of Elements
- A family: Elements in the same group have the same number of valence electrons (number of electrons in the outermost energy level), which corresponds to their group number.
- Highest Main Energy Level: The number of occupied main energy levels (m.e.l) by the electrons corresponds to the period number.
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Electronic Configuration: Elements in the same group have similar outer electronic configurations or last sublevel configurations (LSC).
- s-Block: Elements in Groups 1A & 2A. LSC is Ns1 & Ns2, respectively, where n represents the period number.
- p-Block: Elements in Groups 3A & 8A (except Helium). LSC is Np1 & Np6.
- d-Block: Elements in Groups 3B & 2B. LSC is (n-1)d1 and (n-1)d10.
- f-Block: Lanthanides and Actinides. LSC is (n-2)f1 and (n-2)f14.
Types of Elements
- Metals: Located on the left side and center of the periodic table. They tend to donate electrons and have characteristics like high density, high melting point, luster, and good conductivity of heat and electricity.
- Non-metals: Located on the right side and top of the periodic table. They tend to accept electrons and have characteristics like low density, low melting point, and poor conductivity.
- Metalloids: Elements with properties of both metals and non-metals. These elements are found along the zigzag line on the periodic table.
Trends in Properties
- Metallic Property: The ability of an atom to donate or lose electrons. Increases as you go down a group and across a period (from right to left).
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Atomic Size: The size of an atom. The size increases as you go down a group and decreases as you go across a period.
- Ionic Size An atom becomes an ion by gaining (anion) or losing electrons (cation). Cations are smaller than the neutral atom, and anions are larger than the neutral atom.
- Non-Metallic Property: The ability of an atom to gain or accept electrons. Increases as you go up a group and across a period (from left to right).
- Ionization Energy: The amount of energy required to remove an electron from an atom or ion. Increases as you go up a group and across a period (from left to right).
- Electron Affinity: The energy released when an atom gains an electron to form a negative ion. Increases as you go up a group and across a period (from left to right).
- Electronegativity: The ability for an atom to attract or gain electrons. Increases as you go up a group and across a period (from left to right).
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Description
Explore the development and organization of the periodic table through key historical milestones and the contributions of scientists like Dobereiner, Newlands, Meyer, and Mendeleev. Understand how elements are arranged by atomic number and chemical properties. Test your knowledge of the periodic table's evolution and structure.
