Bonding and Naming Quiz Flashcards

1
Q

Chemical Bond

A

Attractive force between atoms or ions that bind them together as a unit

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2
Q

Covalent Bonding

A

Electrons are shared
Nonmetal plus nonmetal

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3
Q

Ionic Bonding

A

Electrons are transferred
Metal plus nonmetal
Net charge is always zero
Metals transfer to nonmetals

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4
Q

Metallic Bonding

A

Each metal contributes electrons and the electrons flow between atoms
Metal plus metal
Low electronegativity so free to move

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5
Q

Chemical Formula

A

Smallest particle

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6
Q

Formula Unit

A

The chemical formula for an ionic compound, or the simplest whole number ratio of ions present in the crystalline structure
NaCl

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7
Q

Molecular Formula

A

CO2

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8
Q

Compound

A

Two types of elements is binary
More than two types of elements is ternary

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9
Q

Ion

A

One atom is monatomic ion
Two or more atoms is polyatomic ion

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10
Q

Type of Structure

A

Ionic is crystal lattice
Covalent is true molecules
Metallic is “electron sea” or lattice

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11
Q

Physical State

A

Ionic is solid
Covalent is solid, iquid, or gas
Metallic is solid

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12
Q

Melting Point

A

Ionic is high
Covalent is low
Metallic is very high

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13
Q

Solubility in Water

A

Ionic yes
Covalent usually not
Metallic no

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14
Q

Electrical Conductivity

A

Ionic is yes in solution or liquid
Covalent is no
Metallic is yes any form

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15
Q

Other Properties

A

Covalent is odorous
Metallic is malleable, ductile, and lustruous

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16
Q

Polar Covalent

A

Unequal attraction for shared electrons creating partially charged poles or asymmetrical electron density
Overlapping two orbitals and creating polar molecule

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17
Q

Non Polar Covalent

A

Electrons are shared equally or symmetrical electron density
Overlapping orbital

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18
Q

Most Bonds Are

A

A blend of ionic and covalent characteristics

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19
Q

Non Polar Covalent Bond

A

Bonding electrons shared equally between two atoms with no charge
Even sharing

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20
Q

Polar Covalent Bond

A

Bonding electrons shared unequally between two atoms with a partial charge
Uneven sharing

21
Q

Ionic Bond

A

Complete transfer of one or more valence electrons with full charge on resulting ions
Complete transfer

22
Q

Electronegativity

A

The measure of an atom’s ability to attract electrons

23
Q

END

A

Difference in electronegativity which determines bond type
Nonpolar is <0.5 nonmetal + nonmetal
Polar is 0.5 to 1.7 nonmetal + nonmetal
Ionic is >1.7 nonmetal + metal

24
Q

Salts

A

Product of ionic bonding, oppositely charged ions

25
Delocalized
Free to roam about
26
Metal Delocalized
Vacant and nearly empty orbitals of metals overlap
27
Metal Alloys
Formed when metal atoms replace other metal atoms or when smaller metal atoms occupy small spaces between larger atoms
28
True Molecule
A group of two or more atoms held together by chemical bonds, forming the smallest identifiable unit of substance
29
Ionic Compounds Molecule
NOT just a 1:1 ratio Polyatomic ion
30
Properties of Ionic Compounds
DUE TO CRYSTAL LATTICE STRUCTURE Strong High melting and boiling points Conducts electricity in aqueous state Solids at room temperature Brittle
31
Crystalline Solid
A three dimensional network of positive and negative ions mutually attracted to one another
32
Crystal Lattice
The orderly three dimensional arrangement of ions Energy is higher so stronger bond
33
Electron Dot Diagram
Show only the valnce electrons of an atom Place one dot on each side before pairing up Also called ionic compound formations, Lewis dot diagrams, or Lewis structures
34
Helium Electron Dot Diagram
Use two dots on same side
35
Electron Dot Diagram Anion
Put eight dots Brackets around symbol and dots Write charge in top right corner
36
Electron Dot Diagram Cation
Zero dots Brackets around Write charge
37
Comes First
Cations
38
Polyatomic Ions
A group of covalently bonded atoms that bond in such a way that the group has a net charge
39
Lewis Structure for Polyatomic Ions
Count number of valences to be accounted for Draw center atom Show shared pairs of electrons by using a dash instead of dots Central atom will be atom with least electronegativity Add dots so each atom has octet Count to make sure number is correct If ion, add brackets and record charge
40
Lewis Structure for Polyatomic Ions Rules
Central atom will be carbon if present and hydrogen will never be as it only forms one bond Each dash represents two electrons If you have two more electrons than needed, there is a double bond somewhere Four more electrons than needed, triple bond or two double bonds
41
Chemical Formula For Ionic Compound
Represents one formula unit of that compound
42
Oxidation
Charge Many transition elements have more than one possible oxidation state
43
Fixed
Single known charge Anions are always fixed
44
Cation and Anion Rules
Cation first and keeps name Anion changes end to -ide
45
Cross Over Method
Cross the charge number over the subscript of the other atom ALWAYS REDUCE
46
Polyatomic Ions I'm Confused
Ion made up of more than one acts as single charge Treat as one unit Never change subscripts
47
Multivalent
More than one possible oxidation state
48
Type 1 Compound
Binary Metal from columns 1, 2, or 13 and a nonmetal Only one charge or oxidation state