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Merrill Chem. Ch. 10
Pointless rules I really don't care about.
| Question | Answer |
|---|---|
| Elements in the same column have similar... | outer level electron configurations |
| Outer level electron configurations change in a regular way from... | one column to the next |
| Properties are... | periodic |
| What kind of elements have the highest density? | Metals |
| What kind of elements have the lowest density? | Nonmetals existing as gases at room tempereature |
| As the principle quantum number increases, the size of the electron cloud... | increases |
| How does the size of atoms develop as you look down the table? | It increases |
| Why does the size of atoms decrease as you move across a period? | One proton is added with each element, which means the electron cloud is pulled in tighter each time |
| How does the atomic radii of atoms increase? | Top to bottom and right to left |
| The density pattern is... | low-high-low |
| In general, when atoms form to unite compounds... | the compound is more stable than the uncombined atoms |
| Noble gas configurations are particulartly stable because... | the noble gases have filled outer energy levels |
| Chemists discuss the size of ions by referring to their... | ionic radii |
| Metallic ions, on the left and in the center of the table, are formed by... | the loss of electrons |
| Nonmetallic ions, located on the right side of the table, are formed by... | the gain of electrons and are larger than the atoms from which they are formed |
| Metallic ions have an outer level that resembles that of... | the noble gas at the end of the preceding period |
| Non metallic ions have an outer level resembling that of... | the noble gas to the right of the same period |
| The loss of one electron from the metals in Group 1 will give them the same configuration as... | a noble gas |
| What is the oxidation number of Group 1? | 1+ |
| What is the oxidaton number of Group 2? | 2+ |
| What is the oxidation number of Group 13? | 3+ |
| What is the oxidation number of Group 14? | 2+ or 4+ |
| What is the oxidation number of Group 15? | 3- |
| What is the oxidation number of Group 16? | 2- |
| What is the oxidation number of Group 17? | 1- |
| What is the oxidation number of Group 18? | 0 |
| What is ionization energy? | The energy required to remove an electron from an atom |
| What is first ionization energy? | The energy required to remove the loosest electron from an atom |
| What is ionization energy mesured in? | Kilojoules per mole (kJ/mol) |
| How does the first ionization energy change as atomic number increases with a period? | It increases |
| How does the first ionization energy change as atomic number increases with a group? | It decreases |
| First ionization energy can help classify elements into... | metals or nonmetals |
| What kind of first ionization energy do metals have? | Low FIE |
| What kind of first ionization energy do nonmetals have? | High FIE |
| As you go down a column of the periodic table, first ionization energy... | decreases |
| What are two things that tend to lower first ionization energy? | Increased distane of the outer electrons from the nucleus and the sheilding effect |
| What is the sheilding effect? | When inner electrons block the attraction of the nucleus for outer electrons |
| The number of electrons in the outermost sublevel is the same for all elements in a particular... | group |
| Why does first ionization energy increase as you move across a period? | Because the nuclear charge increases |
| What are the four factors that affect ionization energy? | 1. Nuclear Charge- up, up 2. Sheilding Effect- up, down 3. Radius- up, down 4. Sublevel- an electron from a full or half-full sublevel requires additional energy to be removed |
| The first ionization removes a __ electron. | *p electron |
| The second ionization removes a __ electron from a full __ sublevel. | *s electron, s sublevel |
| Are the second and third electrons in different or the same sublevels? | They are in the same |
| Why is the third electron's ionization energy greater? | Because the positive nuclear charge remains constant as you remove electrons |
| What is electron affinity? | The attraction of an atom for an electron |
| The same factors that affect ionization energy also affect... | electron affinity |
| As electron affinity increases, a(n) ____ in ionization energy can be expected. | Increase |
| Metals have ___ electron affinities. | Low |
| Nonmetals have ___ electron affinities. | High |
| As you go down a group, the tendency to gain electrons _____. This is because atoms farther down the column are lerger. (The nucleus is farther from the surface, and attracts the outer electrons ___ strongly.) | Decreases, less |
| As you move across a period (left to right) what happens to the attraction for electrons? | It increases |
| Are positive ions smaller or larger than the atoms from which they are produced? | Smaller |
| Are negative ions smaller or larger than the atoms from which they are produced? | Larger |
| Metals tend to ____ electrons. This means they have positive oxidation numbers. | Lose |
| Nonmetals tend to ____ electrons. This means they have negative oxidation numbers. | Gain |
Created by:
hannahb11
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