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35 Cards in this Set
- Front
- Back
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Define chemical bond |
mutual electrical attraction between nuclei and valence electrons of different atoms that binds atoms together |
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Name the three types of bonds |
ionic covalent hydrogen |
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Ionic bonds |
transfer electrons |
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Covalent bonds |
share electrons |
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Hydrogen bonds |
very weak bonds |
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How can you tell whether something is ionic or covalent? |
By comparing the difference in electronegativity. If it is between 0 and .3, it is nonpolar covalent. If it is between .3 and 1.7, it is polar covalent. If it is larger than 1.7, it is ionic. |
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What makes up a molecule? |
atoms and covalent bonds |
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What is a chemical formula? |
the number of atoms and types of atoms in a molecule |
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What is a molecular formula? |
It is the number and types of molecular compounds . |
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What is bond length? |
Distance between atoms where the potential energy is at a minimum. |
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What is the octet rule? |
Atoms prefer to have eight electrons in their highest energy level. |
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Do you know what a lewis structure is? |
Yes? Great. No? Go look at your notes, buddy. |
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As the number of bonds in a molecule go up, the energy... |
goes up |
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What is a resonance structure? |
It is when the charge of a molecule switches between the atoms. |
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In an ionic compound, the charge should equal... |
Zero |
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What is not in an ionic compound? |
Molecules |
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What is lattice energy? |
Energy given off or taken in to form a crystal lattice. |
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What is a crystal lattice? |
arrangement of atoms in a crystal |
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What are three characteristics of an ionic compound? |
They have a very high melting point, are hard but brittle, breaking in straight lines, and are not conductors of electricity until dissolved in water |
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What is a polyatomic ion? |
A charged group of covalently bonded atoms |
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What causes the many characteristics of metals like luster? |
The electrons are constantly moving between energy levels. |
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Shape determines |
function |
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VSEPR theory stand for? |
Valence-shell electron-pair repulsion |
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Why do molecules bend? |
The lone electron pairs are pushing things around and taking up space. |
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Hydrogen bonding |
highly electronegative atom is attracted to an unshared pair of electrons |
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In order from strongest to weakest, list the types of bonding. |
Ionic, hydrogen, dipole-dipole, london dispersion |
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Describe london dispersion forces |
They are in a molecule where the electrons are swaying from one side to the other, constantly changing which atoms have which charge. These charges can attract other electrons from other molecules, causing a bond to form. It is VERY weak. |
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What type of energy is in an ionic bond? |
Lattice energy |
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What type of energy is in a covalent bond? |
Bond energy |
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What type of energy is in a metallic bond? |
Enthopy of vaporization |
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Describe dipole-dipole. |
It is when one atom in a molecule is more electronegative than the other and thus has a stronger attraction to electrons. This can attract electrons from other molecules, creating a weak bond. |
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As electronegativity difference goes up, ionic character goes |
up. |
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Atoms with covalent bonds have what kind of charge?
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Partial charge |
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As you move from right to left on a periodic table, the strength of a metallic bond |
decreases |
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You will do fine, I promise. |
Don't die; it's bad for your health. |
