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Chem Ch 3
| Question | Answer |
|---|---|
| Who listed the known elements in order of increasing atomic mass, grouping those with similar properties? Precursor to the modern periodic table. | Dmitri Mendeleev |
| Periodic Law | Physical and chemical properties of the elements recur in a systematic and predictable way when the elements are arranged in order of increasing atomic number |
| Who discovered that no two electrons in the same atom can have exactly the same energy | Wolfgang Pauli |
| The Pauli Exclusion Principle | No two electrons in the same atom can have identical sets of quantum numbers |
| We can represent any electron configuration in the following terms: | nl^#e |
| We can also show the arrangement of electrons as: | Orbital diagrams |
| The direction of the arrow in an orbital diagram represents the: | Relative spin of the electron |
| Coulomb's Law | States that energy depends on charge (q) and distance (r) |
| Shielding | The repulsion of one electron by another from the full nuclear charge |
| Effective Nuclear Charge | Zeff |
| Effective nuclear charge equation | Zeff=Z-S |
| Z | Atomic number |
| S | |
| Both shielding and penetration allow for ______ _________ | Energy sublevels |
| Hund's Rule | Electrons fill orbitals that are part of the same n singly first with parallel spins |
| The outermost electrons of an element | Valence electrons |
| The electrons contained in complete energy levels | Core electrons |
| Some irregularities occur when there are enough electrons to half-fill s and d orbitals on a given row. Ex.) Electron configuration for copper: | [Ar] 4s^1 3d^10. This occurs because the 4s and 3d orbitals are very close in energy |
| The periodic table is set up based on ____ and ________ __________ | Size, chemical reactivity |
| Noble gases are: Because their electron configuration is especially stable | Nonreactive, inert |
| Where are metals | Lower left side and middle |
| Metals tend to ____ electrons in chemical reactions | Lose |
| Where are nonmetals | Upper right |
| Nonmetals tend to ____ electrons in reactions with metals to acquire a noble-gas configuration | Gain |
| Where are metalloids | Border the stair-step line |
| What group are alkali metals | 1A |
| What group are alkaline earth metals | 2A |
| What group are halogens | 7A |
| What group are noble gases | 8A |
| Alkali metals | Soft, metallic solids that are highly reactive in water |
| Alkaline earth metals | Higher densities and melting points than alkali metals but are still reactive |
| Halogens | Prototypical nonmetals. Missing 1 electron from having a full shell |
| The chemical properties of elements are largely determined by the number of _______ _________they contain | Valence electrons |
| The distance between 2 nuclei of the same elements at the point of collision is equal to: | The atomic diameter |
| Bonding atomic radius | One-half of the distance between covalently bonded nuclei |
| Bonding atomic radius trend: | Decreases left to right, increases top to bottom |
| Which part of the periodic table has the largest elements? | Bottom/left |
| Ionic size depends upon: | Nuclear charge, number of electrons, and the orbitals in which electrons reside |
| Ion Size trend: | Increases down a column |
| Ionization energy | The amount of energy required to remove an electron from the ground state of a gaseous atom or ion |
| First ionization energy | That energy required to remove the first electron |
| Second ionization energy | That energy required to remove the second electron |
| It requires ____ energy to remove each successive electron | More |
| Trends in first ionization energy | Down a column- less energy required Across a row- harder to remove |
| Firs Ionization energy first discontinuity | Occurs between Groups IIA and IIIA. In this case the electron is removed from a p orbital rather than an s orbital. – The electron removed is farther from the nucleus. – There is also a small amount of repulsion by the s electrons. |
| First Ionization energy second discontinuity | Occurs between Groups VA and VIA – The electron removed comes from a doubly occupied orbital – Repulsion from the other electron in the orbital aids in its removal |
| Electron Affinity | The energy change accompanying the addition of an electron to a gaseous atom |
| Electron Affinity trend: | Becomes more exothermic as you go from left to right across a row |
| Electron Affinity first discontinuity | Occurs between Groups 1A and 2A – The added electron must go in a p orbital, not an s orbital – The electron is farther from the nucleus and feels repulsion from the s electrons |
| Electron Affinity second discontinuity | Occurs between Groups 4A and 5A – Group 5A has no empty orbitals – The extra electron must go into an already occupied orbital, creating repulsion |
| Metals | Have a shiny luster. Solids are malleable and ductile. Good conductors of heat and electricity. Most oxides are ionic solids that are basic. Tend to form cations in aqueous solutions. |
| Nonmetals | Do not have luster. Solids are usually brittle, some hard, some soft. Poor conductors of heat and electricity. Most oxides are molecular substances that form acidic solutions. Tend to form anions or oxyanions in aqueous solution. |
| Metallic character trends: | Decreases left to right, increases top to bottom |
| The greater the number of protons, the _______ the ______ of the ion | Smaller |
| The atomic radius of main-group elements generally increases down a group because.... | The principal quantum number of the valence electrons increases |
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