Chemistry Chapter 7
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| Ions that are formed from one atom are known as _______. | monatomic ions
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| Ionic compounds that absorb water into their solid structure form. | hydrates
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| A group of atoms united by covalent bonds is a(n) ________. | molecule
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| Ionic compounds are always ________. | electrically neutral
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| To form a bond, atoms share _______. | valence electrons
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| Which type of formula best specifies how atoms bond in a molecule? | empirical
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| A positively charged ion attracts a(n) _______. | cation
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| Name 3 properties of Ionic compounds. | -High melting points - Brittle - Good conductors in their liquid state
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| What is the electronegativity when 2 atoms are covalent and nonpolar? | 0.4 or less
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| What is the electronegativity when 2 atoms are covalent and polar? | 0.4< X < 2.0
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| What is the electronegativity when 2 atoms are ionic? | < 2.0
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| Many common ions have the electron configuration of a noble gas. True or False. | True
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| T/F. In a Lew dot diagram, the dots represent [atomic nuclei]. | False. Valence electrons.
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| T/F. Negatively charged ions are [cations]. | False. Anions.
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| T/F. The atoms that make up a sulfate ion are held together by [covalent] bonds. | True.
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| T/F. To emphasize the ratio of ions in a compound, chemists use a [structural formula]. | False. Empirical formula.
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| T/F. Atoms share electrons in an [ionic] bond. | False. Covalent
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| T/F. [Molecules]are composed entirely of ions. | False. Ionic compounds.
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| T/F. The name of the [cation] usually comes first in the name of an ionic compound. | True.
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| T/F. A covalent bond may be polar or [ionic]. | False. Nonpolar
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| Describe an ionic bond. | Chemical bond between a positively charged ion and a negatively charged ion resulting from the transfer of electrons from one bonding atom to another.
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| Describe a covalent bond. | Chemical bond resulting from the sharing of electrons between two bonding atoms.
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| Describe an ionic compound. | A compound that is composed entirely of ions.
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| Describe a cation. | A positively charged ion.
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| Describe an anion. | A negatively charged ion.
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| Describe the octet rule. | The rule that states that atoms tend to gain, lose, or share electrons in order to acquire a full set of valence electrons.
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| Describe monatomic ions. | One atom ions.
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| Describe polyatomic ions. | Two or more atom ions.
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| Describe binary ionic compounds. | Compounds that contain the ions of only two elemens.
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| Describe an empirical formula. | The formula used to denote the ratio of ions in a compound.
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| Describe a molecule. | A group of atoms that are united by covalent bonds.
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| Describe a molecular substance. | A substance that is made of only molecules.
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| Describe a molecular formula. | The formula used to describe the compostion of a molecular compound.
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| Describe a structural formula. | The formula that specifies which atoms are bonded to each other in a molecule.
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| Describe Lewis structures. | Based on the Lewis dot diagram for atoms but used to describe covalent bonds.
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| Describe an unshared pair. | Pairs of electrons in an atom involved in covalent bonds that are not shared in bonds.
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| Single bonds | 2 atoms share exactly one pair of electrons
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| double bonds | consists of two pairs of shared electrons
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| triple bonds | consists of three pairs of shared electrons
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| polar | when one atom is significantly more electronegative than another in a covalent bond
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| nonpolar | when 2 atomshave similar or equal electronegativites and they both exert approximately equal pull on the electrons in the bond.
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| hydrates | ionic compounds that absorb water into their solid structures
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| anhydrous substances | water-free substances
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| Why are many elements more stable as ions than they are as atoms? | In their ionic form, they have the same electron configuration as the previous noble gas, which are unreactive.
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| Why are some covalent bonds polar and others nonpolar | Because the elements have varying electronegativites.
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