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Honors Chemistry > Unit 1 > Flashcards

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
Q

Expanded Octets

A

P
S
Xe

26
Q

Can Form Covalent Bonds

A

Beryllium
Yuh

27
Q

Can Form With Expanded Octets

A

Periods 3
And below

28
Q

Valence Electrons

A

Across
Yuh

29
Q

Lewis Structure Rules

A

Count
Find middle
Set up
Add to middle then ends
Create bonds
Count again

30
Q

HONC

A

Hydrogen and halogens form one bond never central atom
Oxygen forms two bonds
Nitrogen forms three bonds
Carbon forms four bonds

31
Q

Lone Pairs

A

Repel more strongly because they take up more space
Reduce bond angle

32
Q

REMEMBER

A

Don’t forget to check diatomic
Ionic can’t share bonds

33
Q

Dipoles

A

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
Q

Polarity of Molecules Can Affect

A

Many of their other properties
Such as their solubility, boiling and melting points, and their odor

35
Q

Electronegativity Symbol

A

∆EN
Yuh

36
Q

Determining Molecular Polarity One Central Atom

A

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
Q

Determining Molecular Polarity Two or More Central Atoms

A

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
Q

Molecule Can Still Be Nonpolar If

A

Overall pull still cancels out
Bonds are still evenly spaced
Magnitude is what matters

39
Q

Less Electronegative

A

Named first
Yuh

40
Q

Bent Shape Ensures

A

Dipole moments don’t cancel out
Yuh

41
Q

Resonance Structure

A

Set of two or more electron dot diagrams of a single polyatomic Including fractional bonds and fractional charges

42
Q

Molecular/Geometric Structure

A

Three dimensional arrangement of atoms within a molecule
Including the bond lengths, angles, and relative positions of each atom

43
Q

Type I Binary Compound

A

Has cation that has only one charge
Metals in group one and group two and aluminum in group thirteen

44
Q

Type II Binary Compound

A

Has cation that has multiple charges
All other metals that are not type one

45
Q

Type I Ternary Compound

A

Contains a metal with fixed oxidation Bonded to polyatomic ion

46
Q

Type II Ternary Compound

A

Contains a multivalent metal
Bonded to a polyatomic ion

47
Q

Oxyanion

A

A negatively charged polyatomic ion
That contains oxygen

Honors Chemistry (13 decks)

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