Structure and Properties of Ionic and Covalent Compounds Flashcards

1
Q

Force of attraction between any atoms in a compound

A

Chemical bonding

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2
Q

Interactions involving __________ that are responsible for the chemical bond

A

valence electrons

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3
Q

A way to represent atoms using the element symbol and valence electrons as dots

A

Lewis Symbols

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4
Q

In Lewis symbols, the number of dots used corresponds directly to the number of ______ located in the _____ of the atoms of the element

A

valence electrons, outermost shell

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5
Q

attractive force due to the transfer of one or more electrons from one atom to another

A

Ionic bond

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6
Q

Reason for attraction between atoms

A

The attraction is due to the
opposite charges of the ions

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7
Q

attractive force due to the sharing of electrons between atoms

A

Covalent bond

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8
Q

is a symmetrical 3-D structural arrangements of atoms, ions or molecules (constituent particle) inside a crystalline solid as points

A

Crystal lattice

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9
Q

Compounds containing covalent bonds are called???

A

covalent compounds or molecules

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10
Q

Bonds of diatomic elements

A

covalent bond

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11
Q

A physical property of compounds which relates other physical properties such as melting and boiling points, solubility, and intermolecular interactions between molecules.

A

Bond polarity

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12
Q

bonds made up of unequally shared electron pairs

A

Polar covalent bonding

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13
Q

bonds made up of equally shared electrons pairs

A

Nonpolar covalent bonding

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14
Q

Electronegativity Difference Range of nonpolar covalent bond

A

0.0 - 0.4

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15
Q

Electronegativity difference range of polar covalent bond

A

0.5 - 2.0

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16
Q

Electronegativity difference range of ionic bond

A

greater than 2.0

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17
Q

Chemical bond: metal + nonmetal

A

ionic

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18
Q

Chemical bond: 2 nonmetals

A

covalent

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19
Q

In ionic bond, electrons are _____

A

transfered

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19
Q

Chemical bond: boiling and melting point of ionic bond

20
Q

In covalent bonds, electrons are ____

21
Q

the assignment of a correct and unambiguous name to each and every chemical compound

A

Nomenclature

22
Q

2 naming systems

A
  • ionic compounds
  • covalent compounds
23
Q

representation of the fundamental compound using element symbols and numerical subscripts

A

Chemical formula

24
Method: the charge of each ion is crossed over to become a subscript of the other ion
Crisscross method
25
How to name representative metal
Metal (element name) + nonmetal (stem name of nonmetal + suffix -ide)
26
2 names for transition metals
* stock name * classical name
27
How to form stock name?
Use element name + Roman numeral that represent the charge of the cation + anion stem + -ide
28
How to form classical name (common name)
Use of Latin name stem + the suffix -ous (lower charge) or -ic (higher charge) of the cation + anion stem + -ide
29
Composed of two or more atoms that are covalently bonded together with an overall positive or negative charge
Polyatomic ion
30
one pair of electrons is shared between two atoms
Single bond
31
two pairs of electrons are shared between two atoms
double bond
32
three pairs of electrons are shared between two atoms
triple bond
33
- the amount of energy required to break a bond holding two atoms together
Bond energy
34
Decreasing bond energy
triple bond > double bond > single bond
35
Distance separating the nuclei of two adjacent atoms
Bond length
36
Decreasing bond length order
Single bond > double bond > triple bond
37
A property of a compound having two or more possible Lewis structures that contribute to the real structure.
Resonance structures
38
- The possible structures do not accurately represent the structure of the compound experimentally.
Resonance structures
39
- less than eight electrons around an atom other than H
Incomplete octet
40
if there is an odd number of valence electrons, it is not possible to give every atom eight electrons
Odd electron
41
an element in the 3rd period or below may have 10 and 12 electrons around it
Expanded octet
42
VSEPR theory
Valence Shell Electron Pair Repulsion Theory
43
used to predict the shape of the molecules
VSEPR theory (Valence Shell Electron Pair Repulsion Theory)
44
attractive forces within molecules (chemical bonds).
Intramolecular forces
45
attractive forces between molecules (hydrogen bonding, Van der Waals forces, London dispersion forces, etc.)
Intermolecular forces
46
the maximum amount of solute that dissolves in a given amount of solvent at a specific temperature
Solubility
47
– has direct proportionality to B.P. and M.P
Molecular mass
48
polar molecules have higher B.P. and M.P. than nonpolar molecules due to their strong intermolecular forces of attraction
Polarity