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Chem Unit 2
| Question | Answer |
|---|---|
| Who first published the classification of the elements that is the basis of our periodic table today? | Mendeleev |
| By what property did Mendeleev arrange the elements? | Increasing atomic mass and similar chemical and physical properties |
| By what property did Moseley suggest that the periodic table be arranged? | Increasing atomic number |
| What is a period? How many are there in the periodic table? | A horizontal row; 7 |
| What is a group (also called a family)? How many are there in the periodic table? | A vertical column; 18 |
| What are the transition elements? | The metals of the d-block |
| What are the Group 1 elements called? | The alkali metals |
| What are the Group 2 elements called? | The alkaline earth metals |
| What are the Group 17 elements called? | The halogens |
| What are the Group 18 elements called? | The noble gases |
| Why do all the members of a group have similar properties? | Same number of valence electrons |
| Where, generally, are the metals located on the periodic table? List some of the physical properties of metals. | The metals are to the left of the stair-step. Metals are solids at room temperature (except Hg), they are lustrous, malleable, ductile, and they are excellent conductors of heat and electricity. |
| Where, generally, are the nonmetals located on the periodic table? List some of the physical properties of non-metals. | The nonmetals are to the right of the stair-step. Non-metals can be solids, liquids, or gases at room temperature. They are not lustrous, not malleable, not ductile, and do not conduct electricity. Solids are brittle. |
| What is the main characteristic property of the noble gases? | They are inert (unreactive). |
| What is the main characteristic property of the semi-metals? | They are good semi-conductors. |
| What type of element reacts violently with water? | Alkali metal |
| What type(s) of element(s) produce basic solutions when they react with water? | Alkali and Alkaline Earth metals |
| What type of element has full s and p orbitals? | Noble gases |
| What type of element is found in the d block of the periodic table? | Transition metals |
| What type of element is found in the f block of the periodic table? | Inner transition metals |
| What type of element pairs nicely with the elements of group 1 to form salts? | Halogens |
| What type of element has 2 valence electrons? | Alkaline earth metals, transition metals, inner transition metals |
| What type of element is the most reactive nonmetal? | halogens |
| What type of element exists as diatomic molecules in nature? | halogens |
| What type of element has 1 valence electron? | Alkali metal |
| what happens to the strength of the Coulombic attraction between the positive nucleus and the negatively charged valence electrons as you travel down a group. | The Coulombic attraction weakens as you travel down a group because of the addition of new energy levels which puts more distance between the nucleus and the valence electrons. |
| what happens to the strength of the Coulombic attraction between the positive nucleus and the negatively charged valence electrons as you travel across a horizontal row (period). | The Coulombic attraction strengthens as you travel across a horizontal row because more protons and electrons are added, but no new energy levels are added. |
| Define “atomic radius” | The distance between the center of the nucleus and the electrons in the outermost energy level |
| Moving from top to bottom of a group, what happens to the atomic radius as you go down the column? | Atomic radius increases as you travel down a group due to the addition of new energy levels that weakens the Coulombic attraction between the positively charged nucleus and negatively charged valence electrons. |
| Why does the atomic radius change going down column? | Atomic radius increases as you travel down a group due to the addition of new energy levels that weakens the Coulombic attraction between the positively charged nucleus and negatively charged valence electrons. |
| Moving from left to right across a period, what happens to the atomic radius? | Atomic radius increases as you travel down a group due to the addition of new energy levels that weakens the Coulombic attraction between the positively charged nucleus and negatively charged valence electrons. |
| Why does the atomic radius change left to right? | Atomic radius increases as you travel down a group due to the addition of new energy levels that weakens the Coulombic attraction between the positively charged nucleus and negatively charged valence electrons. |
| Define the term ionization energy. | The energy required to remove an electron from the valence shell of an atom |
| What is the general trend of ionization energy as you go from left to right across the periodic table? Explain this trend in terms of atomic structure. | Ionization energy increases as you travel across a period due to the strengthening Coulombic attraction between the positively charged nucleus and negatively charged valence electrons. |
| What is the general trend of ionization energy as you go down a group on the periodic table? Explain this trend in terms of atomic structure. | Ionization energy decreases as you travel down a group due to the weakening Coulombic attraction between the positively charged nucleus and negatively charged valence electrons. |
| When an atom becomes an anion, what happens to its radius? Explain. (Hint: Think about how the atomic structure changes.) | It becomes larger because it is gaining an electron |
| When an atom becomes a cation, what happens to its radius? Explain. (Hint: Think about how the atomic structure changes.) | Cations are smaller than neutral atoms of the same element. They are formed when atoms lose electrons. |
| What is electronegativity? | The ability of an atom to attract electrons to itself in a chemical bond |
| What is the general trend of electronegativity as you go from top to bottom within a column in the periodic table? Explain this trend in terms of atomic structure. | Electronegativity decreases because of the addition of new energy levels that weaken the Coulombic attraction. |
| What is the general trend of electronegativity as you go left to right across the periodic table? Explain this trend in terms of atomic structure. | Electronegativity increases because of the strengthening Coulombic attraction that results as more protons and electrons are added, but no new energy levels are added. |
Created by:
wmke8