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54 Cards in this Set
- Front
- Back
The force that holds two atoms together is called a |
Chemical Bond |
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A chemical bond may form by the attraction of the positively charged _ of one atom for the negatively charged _ of another atom, or by the attraction of charged atoms, _ |
Nucleus, Electrons, Ions |
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The electrons in the outermost energy level are _ |
Valence Electrons |
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The _ are a family of elements that have very little tendency to react |
Noble Gases |
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An element that is stable full outer energy level is also called a stable _ |
Octet |
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The relatively stable electron structures developed by loss of electrons in certain elements of groups 3, 4, 13, and 14 are called _ |
Pseudo-Noble Gas formations |
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A positively charged ion is called a _ |
Cation |
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The ending -ide is used to designate an _ |
Anion |
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An ionic bond is _ |
A force that holds together atoms that are oppositely charged |
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The formula unit of an ionic compound shows the _ |
Simplest ratio of the ions |
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The overall charge of a formula unit for an ionic compound _ |
Is always zero |
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Ionic compounds generally occur between _ |
Metals and Nonmetals |
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Salts are examples of _ |
Ionic Compounds |
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A three-dimensional arrangement of particles in an ionic solid is called a _ |
Crystal Lattice |
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In a crystal lattice of an ionic compound _ |
Ions are surrounded by ions of the opposite charge |
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What is the relationship between lattice energy and the strength of the attractive force holding ions in place? |
The more negative the lattice energy is, the greater the force. |
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The formation of a stable ionic compound from ions _ |
Is always exothermic |
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In electron transfer involving a metallic atom and a nonmetallic atom during ion formation, which of the following is correct? |
The nonmetallic atom gains electrons from the metallic atom. |
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Ionic compounds have a _ melting point |
High |
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Ionic compounds have a _ boiling point |
High |
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Ionic compounds are hard/soft |
Hard |
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Ionic compounds are flexible/brittle |
Brittle |
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Electrical conductivity in the solid state |
Poor |
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Electrical conductivity in the liquid state |
Good |
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Electrical conductivity when dissolved in water
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Good |
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Does the crystal lattice of ionic compounds affect their melting and boiling points? |
Yes |
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Is lattice energy the energy required to separate the ions of an ionic compound? |
Yes |
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Is the energy of an ionic compound higher than that of the separate elements that formed it? |
No |
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Do large ions tend to produce a more negative value for lattice energy than smaller ions do? |
No |
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Do ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges? |
Yes |
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A one atom ion is called _ |
Monatomic |
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The charge of a monatomic ion is equal to the atoms _ |
Oxidation number |
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The oxidation number is the number of _ transferred to or from the atom to for the ion. |
Electrons |
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In ionic compounds, the sum of the charges of all the ions equals _ |
Zero |
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Ions made up of more than one atomic are called _ ions |
Polyatomic |
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If a polyatomic ion is negatively charged and includes one or more oxygen atoms, it is called an _ |
Oxyanion |
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If two oxyanions form that contain different numbers of oxygen atoms, the name for the ion with more oxygen atoms ends with the suffix _ |
Ate |
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The name for the ion with fewer oxygen atoms ends with the suffix _ |
Ite |
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In the chemical formula for any ionic compound, the chemical symbol for the _ is written first |
Cation |
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After the cation the chemical symbol for _ is put. |
Anion |
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A _ is a smaller number used to represent the number of ions of a given element in a chemical formula |
Subscript |
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Subscripts are written to the _ of the symbol for the element |
Lower right |
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If no number appears, the assumption is that the number equals _ |
One |
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ClO2- |
Chlorite |
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ClO4- |
Perchlorate |
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ClO- |
Hypochlorite |
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Cl- |
Chloride |
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ClO3- |
Chlorate |
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The name of the model of metallic bonding is the _ |
Electron Sea Model |
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The electrons in a metallic solid are described as delocalized because _ |
They are free to move from one atom to another |
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The electrons from the metal make up the delocalized electrons are _ |
Valence Electrons |
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The metal atoms are |
Cations |
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Metallic ions differ from the ions that exist in ionic solids because the |
Electrons are not completely lost by the metal atoms like in a ionic solid |
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The reason why the metal atoms hold together in a solid is because they are |
Bonded by the oppositely charged electron sea that surrounds them
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