Term
| What are actinide series? |
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Definition
| in the periodic table, the f-block elements from period 7 that follow the element actinuim |
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Term
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Definition
| Group 1 elements, except for hydrogen, they are reactive and usually exist as compounds with other elements |
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Term
| What are alkaline earth metals? |
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Definition
| Group 2 elements in the modern periodic table and are highly reactive |
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Term
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Definition
| a vertical column of elements in the periodic table arranged in order of increasing atomic number; also called a family |
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Term
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Definition
| Highly reactive elements in group 7A or 17 |
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Term
| What are inner transition metals? |
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Definition
| A type of group B element that is contained in the f-block of the periodic table and is characterized by a filled outermost orbital, and filled or partially filled 4f and 5f orbitals |
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Term
| What s the lanthanide series? |
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Definition
| In the periodic table, the f-block elements from period 6 that follow the element lanthanum |
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Term
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Definition
| an element that is solid at room temperature and are located on the left of the zig-zag line, but not on it |
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Term
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Definition
| an element that has physical and chemical properties of both metals and nonmetals, located on either side of the zig-zag line |
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Term
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Definition
| an extremely unreactive group 8A(18) element |
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Term
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Definition
| Element that is gernerally a gas, or a dull, brittle solid and is a poor conductor of heat and electricity |
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Term
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Definition
| a horizontal row of elements in the modern periodic table |
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Term
| What is the Periodic Law? |
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Definition
| States that when the elements are arragned by increasing atomic number, there is a periodic repetition of their properties |
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Term
| What are representative elements? |
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Definition
| elements from groups 1,2,and 13-18 in the modern periodic table, possessing a wide range of chemical and physical properties(all but the transition and inner transition metals) |
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Term
| What are transition elements? |
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Definition
| elements in groups 3-12 of the modern periodic table and are further divided into transition metals and inner transition metals |
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Term
| What is a transition metal? |
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Definition
| An element in groups 3-12 that is contained in the d-block of the periodic table and, with some exceptions, is characterized by a filled outermost s orbital of energy level n and filled or partially filled d orbitals of energy level n-1 |
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Term
| What is electronegativity? |
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Definition
| Indicates the relative ability of an element's atoms to attract electrons in a chemical bond |
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Term
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Definition
| an atom or bonded group of atoms with a positive or negative charge |
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Term
| What is ionization energy? |
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Definition
| the energy required to remove an electron from a gaseous atom |
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Term
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Definition
| States that atoms lose, gain, or share electrons in order to acquire the stable electron configuration of a noble gas |
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Term
| What are some properties of metals? |
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Definition
| malleable and ductile, good conductor of electricity, lustrous, silver or white in color, good conductor of heat |
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Term
| What are some characteristics of nonmetals? |
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Definition
| solids, liquids or gases; do not conduct electricity, do not conduct heat; do not react with acids; likely brittle if solid |
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Term
| What are some characteristics of metalloids? |
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Definition
| combine properties of metals and nonmetals |
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Term
| In the element [Kr]5s24d10 What is the period? What is the block? What is the group? |
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Definition
| The period is 5, the block is d, and the group is 12 |
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Term
| What groups are in block "s"? |
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Definition
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Term
| What groups are in block d? |
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Definition
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Term
| What groups are in block p? |
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Definition
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Term
| What groups are in f block? |
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Definition
| the inner transition metals |
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Term
| As you go across the period, What does atomic radii do? |
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Definition
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Term
| As you go down the group, What does the atomic radii do? |
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Definition
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Term
| Why does the atomic radii decrease across a period? |
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Definition
| the greater the atomic number the more protons that are in the nucleus which causes a greater positive charge to pull in the electrons |
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Term
| Why does the atomic radii increase as you go down the group? |
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Definition
| because the farther down you go, the more energy levels you have |
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Term
| What happens to the ionization energy as you go down the period? as you go across the period? |
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Definition
| down-ionization energies decrease, across-ionization energies increase |
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Term
| What happens to the ionic radius as you go down the group? |
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Definition
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Term
| Why do nonmetals have a greater ionic radius than their atomic radius? |
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Definition
| because of the electron's tendency to repel one another; when an electron is added, the electrons push away from one another |
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Term
| What does electronegativity do when you go down the period? across the period? |
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Definition
| down- it decreases; across-it increases |
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Term
| What scientist came up with the Law of octaves which says the there is a periodic repetition in the elements? |
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Definition
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Term
| What scientist came up with the Law of octaves which says the there is a periodic repetition in the elements? |
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Definition
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Term
| What 2 scientists organized the periodic table according to increasing atomic masses? |
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Definition
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Term
| Who came up with the modern periodic table today, and what is it based on? |
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Definition
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