Chemistry chapter 10
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Created by:
smileabby2014 on December 27, 2011
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27 terms
Terms | Definitions |
|---|---|
 defined as half of the distance between the nuclei of identical atoms that are bonded together | atomic radii |
| What is the trend across periods for ATOMIC RADII | it decreases, because the pull from the nucleus due to increased positive charge |
| What is the trend down groups for ATOMIC RADII | it increases, because of the increase of energy levels which get further and further out |
| the energy needed to remove an electron from a neutral atom | Ionization Energy |
| What is Ionization Energy measured in | kJ/mol |
| Any process that results in the formation of an ion | ionization energy |
| What is IE used to compare | It is used to compare how easily different types of atoms give up electrons |
| What is IE basically? | atom + (energy) ----> A+[cation] + electron |
| What kind of IE do metals have | low |
| What kind of IE do nonmetals, especially noble gases have | higher |
| When you move down groups, what happens to the IONIZATION ENERGY | IE decreases because electrons are removed easier since they are further from the nucleus and other electrons shield the outer electrons from the nuclear charge |
| When you move additional electrons, what is it called? | second IE, third IE, etc. |
| Which is harder to remove, the first or second electron | the second because there are less electrons to shield the remaining electrons from the nuclear forces, in continues on... |
| What are the factors that affect IE values | nuclear charge, shielding effect, radius, sub-level [read about these and know chart in book] |
| the energy change that occurs when an electron is acquired by a neutral atom or how much an atom wants an electron | Electron Affinity |
| What is electron affinity measured in | kJ/mol |
| Most atoms _________ energy when they gain an electron | release, like atom + electron ----> amion + energy, exothermic |
| What is the least popular way to gain an electron | Like an endothermic reaction, Atom + electron + energy ----> anion |
| Explain Halogens and Electron Affinity | they gain electrons so rapidly because of their affinity, this is why they are so reactive |
| Which groups have negative EA | alkaline earth metals, noble gases |
| As you move across a period, what is the pattern for Electron Affinity | it mostly increases |
| As you move down a group, what is the pattern for electron affinity | they sometimes increase, sometimes decrease |
| The radius of an atom's ion | Ionic Radii |
| When the atom's ion is a cation+, it is _____ | smaller than its atom |
| When the atom's ion is a anion-, it is _________ | larger than its atom |
| As you move across a period, what is the pattern for ionic radii | it varies |
| As you move down a group, what is the pattern for ionic radii | it increases |
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