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Chemistry > Test 6 > Flashcards

Test 6 Flashcards

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1
Q

what are good examples of atoms with stable electron configurations

A

noble gases

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2
Q

bonding usually __ energy as the atom’s electron configurations attain lower energy states

A

releases

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3
Q

why do atoms with more than 4 valence electrons tend to gain electrons?

A

they have relatively high electron affinities

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4
Q

__ is the tendency of an object to form 2 localized regions of opposite character

A

polarity

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5
Q

can a completely ionic bond result from electron transfer? why? why not?

A

no, that would imply that the donor atom had no affinity for the donated electrons

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6
Q

what is a bonding pair of electrons and where are they found?

A

the two shared electrons that make up a pair. they are in between the nuclei

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7
Q

what is electrostatic force

A

the force exerted between electrical charges

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8
Q

name the natural diatomic elements

A

Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine

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9
Q

when using Lewis structures, a __ is substituted for the bonding pair to simplify the diagram

A

dash

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10
Q

in a Lewis structure a dash represents how many electrons?

A

2

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11
Q

The element with the most __ electrons will likely be the central atom

A

bonding sites/unpaired electrons

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12
Q

most polyatomic ions are __, formed by acquiring additional electrons to make up their octet

A

anions

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13
Q

how many atoms can hydrogen have

A

2

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14
Q

what is the hardest natural substance known?

A

diamond

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15
Q

the melting points of ionic compounds are at least__, illustrating just how __ their bonds are. describe ionic compounds

A

800*C
strong
dense, brittle, and hard solids

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16
Q

An __ is a mixture of a metal’s atoms with another element and has metallic properties

A

alloy

17
Q

what kind of energy moves quickly through metallic objects

A

thermal

18
Q

the shape of a metal object can be changed by hammering or stretching __ significantly affecting its __

A

without

strength

19
Q

covalent bonds

A

Two atoms held together by their mutual attraction for the same pair of electrons. It usu- ally involves two nonmetals

20
Q

ionic bonds

A

The attraction and electron transfer between two oppositely charged ions in a solid. It usually involves a metal and a nonmetal.

21
Q

metallic bonds

A

A communal sharing of electrons between metal atoms.

22
Q

A force of attraction produced by transferring or sharing electrons that holds atoms together in compounds.

A

chemical bonds

23
Q

states that an atom tends to gain, lose, or share electrons until its outer level s and p orbitals are filled with eight electrons. This activity gives an element the electron configuration and stability of a noble gas.

A

octet rule

24
Q

in covalent bonding…

A

electrons are shared

25
Q

CNN

A

covalent nonmetal nonmetal

26
Q

IMN

A

ionic metal nonmetal

27
Q

MMM

A

metallic metal metal

28
Q

guidelines for creating Lewis structures

A
  1. Lewis structures illustrate only compounds consisting of covalent bonds.
  2. Electron sharing occurs when one nonmetal atom bonds with another (e.g., hydrogen and fluorine) or when two identical nonmetal atoms bond (e.g., fluorine and fluorine).
  3. Each nonmetal generally forms covalent bonds to achieve eight electrons in its valence shell, including bonding and nonbonding electrons. Hydrogen is a major exception since its valence shell holds only two electrons.
  4. Electrons are normally shared in pairs since two electrons of opposite spin occupy empty orbitals.
  5. Polyatomic molecules, which contain three or more atoms, have one or more central atoms bonded to surrounding atoms. Since hydrogen can share only one pair of electrons, it can never be the central atom in a polyatomic molecule. Atoms with valence structures similar to Group 14 atoms (the carbon family) are more likely to be the central atom in a polyatomic molecule.
  6. The number of valence electrons for nonmetals (except hydrogen) can be predicted by the formula valence e– = group number – 10. The number of covalent bonds in which nonmetals can participate is predicted by the formula covalent bonds = 8 – valence e–
29
Q

A group of atoms that maintains a constant electrical charge while existing as a unit in a wide variety of chemical reactions

A

polyatomic ion

30
Q

An extensive three-dimensional structure that represents the regular pattern of atoms or ions

A

crystal lattice

31
Q

A theory that offers an explanation of how metals bond: the valence electrons of atoms are said to be freely shared among all atoms

A

electron sea theory–associated with metallic bonds

32
Q

An electron that can move between several different bonds

A

delocalized electron

33
Q

why do electrons rearrange during bonding?

A

to maximize stability

Chemistry (32 decks)

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