Unit 1 Flashcards

1
Q

Bond Formations

A

Ionic transferred from metal to nonmetal
Covalent shared between two nonmetals
Metal delocalized among metal atoms

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2
Q

Physical States

A

Ionic solid
Covalent solid, liquid, or gas
Metal solid

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3
Q

Melting Points

A

Ionic high
Covalent low
Metal very high

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4
Q

Solubility

A

Ionic yes
Covalent usually not
Metal no

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5
Q

Electrical Conductivity

A

Ionic yes solution or liquid
Covalent not
Metal yes any form

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6
Q

Other Properties

A

Ionic no
Covalent odorous
Metal malleable, ductile, lustrous

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7
Q

Salts

A

Product of ionic bonding
Oppositely charged ions

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8
Q

Metal Alloys

A

Formed when metal atoms replace other metal atoms
Or when larger metal atoms occupy small spaces between larger atoms

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9
Q

True Molecule

A

A group of two or more atoms held together by chemical bonds
Forming the smallest identifiable unit of substance

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10
Q

Properties of Ionic Compounds

A

Bonds are very strong
High melting and boiling point
Does not conduct electricity in solid state but aqueous state
Solids at room temperature
Made of metal and nonmetal

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11
Q

Aqueous

A

Dissolved in water
Changes properties

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12
Q

Crystalline Solid

A

Three dimensional network of positive and negative ions
Mutually attracted to one another

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13
Q

Crystal Lattice

A

The orderly three dimensional arrangement
Ions

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14
Q

Electron Dot Diagrams

A

Place one dot on each side before pairing up
Besides helium which uses two dots on same side

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15
Q

Electron Dot Diagram Cation

A

Zero dots to represent losing level
Brackets and charge

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16
Q

Electron Dot Diagram Anion

A

Eight dots to represent octet
Brackets and charge

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17
Q

Formation of Ionic Compounds

A

Write metal first
Then nonmetal

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18
Q

Lattice Energy

A

Higher
Means stronger bond

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19
Q

Polyatomic Ions

A

Group of covalently bonded atoms that bond in such a way that the group has a net charge

20
Q

Covalent Naming Rules

A

Name first element fully using prefix besides one
Second element always change to -ide and ad prefix

21
Q

Acid Naming Rules

A

Start with hydrogen
No oxygen use hydro-
Find number of hydrogen based on charge of anion
Use other element or polyatomic ion name
-ate to -ic
-ite to -ous

22
Q

Binary Acid

A

Second element nonmetal
Root of second elements name follows prefix
Ends with -ic acid

23
Q

Writing Acidic Formulas

A

No hydro- tells oxyacid
Change -ic to -ate and -ite to -ous
Write symbol with their charges
All begin with H+1
Add the nonmetal
Crossover and reduce

24
Q

Incomplete Octet

A

Hydrogen only forms one bond
Boron only forms three bonds
Beryllium only forms two bonds

25
Expanded Octets
P S Xe
26
Can Form Covalent Bonds
Beryllium Yuh
27
Can Form With Expanded Octets
Periods 3 And below
28
Valence Electrons
Across Yuh
29
Lewis Structure Rules
Count Find middle Set up Add to middle then ends Create bonds Count again
30
HONC
Hydrogen and halogens form one bond never central atom Oxygen forms two bonds Nitrogen forms three bonds Carbon forms four bonds
31
Lone Pairs
Repel more strongly because they take up more space Reduce bond angle
32
REMEMBER
Don't forget to check diatomic Ionic can't share bonds
33
Dipoles
Polar bonds constitute Polarity of individual polar bond between atoms Or he net polarity of a polar molecule that may have several polar covalent bonds within it Or the polar molecule itself
34
Polarity of Molecules Can Affect
Many of their other properties Such as their solubility, boiling and melting points, and their odor
35
Electronegativity Symbol
∆EN Yuh
36
Determining Molecular Polarity One Central Atom
Lone pairs means polar No lone pairs but terminal atoms on same element means nonpolar No lone pairs and no terminal atoms means polar
37
Determining Molecular Polarity Two or More Central Atoms
Lone pairs means polar No lone pairs but central and terminal atoms on same element means nonpolar No lone pairs but central atoms on same element and no terminal atoms on same element means polarity depends on symmetry No lone pairs and no central atoms means polar
38
Molecule Can Still Be Nonpolar If
Overall pull still cancels out Bonds are still evenly spaced Magnitude is what matters
39
Less Electronegative
Named first Yuh
40
Bent Shape Ensures
Dipole moments don't cancel out Yuh
41
Resonance Structure
Set of two or more electron dot diagrams of a single polyatomic Including fractional bonds and fractional charges
42
Molecular/Geometric Structure
Three dimensional arrangement of atoms within a molecule Including the bond lengths, angles, and relative positions of each atom
43
Type I Binary Compound
Has cation that has only one charge Metals in group one and group two and aluminum in group thirteen
44
Type II Binary Compound
Has cation that has multiple charges All other metals that are not type one
45
Type I Ternary Compound
Contains a metal with fixed oxidation Bonded to polyatomic ion
46
Type II Ternary Compound
Contains a multivalent metal Bonded to a polyatomic ion
47
Oxyanion
A negatively charged polyatomic ion That contains oxygen