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ch5 struct Flashcards

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1
Q

3 types of bonding

A

Covalent, Metallic, Ionic

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2
Q

5 structures

A
  1. Giant Ionic Lattice Structure
  2. Giant Molecular Structure
  3. Giant Metallic Lattice Structure
  4. Simple Molecular Structure
  5. Macromolecules
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3
Q

Match these respective bonding to the structure

  1. G I L S
  2. G M S
  3. G M L S
  4. SMS
  5. M
A

Giant Ionic Lattice Structure - Ionic Bonding
Giant Molecular Structure - Covalent Bonding
Giant Metallic Lattice Structure - Metallic Bonding
Simple Molecular Structure - Covalent Bonding
Macromolecule - Covalent Bonding

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4
Q

Diamond Structure vs Silicon Dioxide Structure (1 similarity, 1 difference)

A

SIMILARITY: Diamond and Silicon Dioxide Structure:
Tetrahedral, arrangement

DIFFERENCE:
Diamond: Carbon, atoms, bonded, four, other, carbon, atoms

Silicon Dioxide: Oxygen, atom, bonded, two, silicon, atoms
Silicon, atom, bonded, four, oxygen, atoms

for siO2 (silicon dioxide)

1 si bonded to 2*2 = 4 oxygen atoms

1 oxygen bonded to 1*2 = 2 silicon atoms

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5
Q

Diamond Industrial Uses

A
  1. Used as drill bits
  2. Cutting tools for glass

**Not accepted: Used as jewelry

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6
Q

Is pencil lead made out of Lead (Pb) or Graphite?

A

Graphite

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7
Q

Is silicon dioxide (Sand) M________ or GMS?

A

Giant Molecular Structure (tetrahedral arrangement)

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8
Q

2 types of forces

A
  • Weak intermolecular Forces of attraction
  • strong electrostatic forces of attraction
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9
Q

Is Pencil Lead M or GMS? What is its arrangment?

A

Graphite: Giant Molecular Structure

Structure: Within, each, layer, carbon atoms, arranged, form, hexagonal, rings

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10
Q

Graphite forces and bonding

A

Forces: Weak, intermolecular, forces, of attraction, exist, between, hexagonal, flat, layers of atoms.

Bonding: strong, covalent, bonds, exist, between, atoms

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11
Q

cube

Giant Ionic Lattice Structure forces and bonds and structure

A
  1. Each, ion, surrounded, 6, other, ions
  2. Strong, ionic, bonds
  3. Cations, anions, held together, strong electrostatic forces

** A cube has 6 faces. Thus, each atom is surrounded by 6 other atoms

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12
Q

Ionic bonds are formed by?

A

Metal, nonmetal, transferring, electrons

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13
Q

Derive

Giant Ionic Lattice Structure - Physical Properties

A
  1. Ionic compounds, typically dissolve -> water,
  2. does not dissolve, organic solvent
  3. hard, brittle
  4. high melting point boiling point
  5. conducts electricity+heat, molten, aqueous state

GILLS of fish like water hate other solvents

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14
Q

Giant Molecular Structure physical properties

A
  1. High melting, boiling, points
  2. Doesn’t, conduct, electricity
  3. insoluble, organic solvent, insoluble, water
  4. Very hard

GMS, GMLS hates everything, does not dissolve in anything

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15
Q

Giant Metallic Lattice Structure physical properties

A
  1. High Boiling, melting, points
  2. Good, conductor, electricity
  3. Malleable, ductile, soft
  4. Not soluble in water or organic solvent

For no 4:
Metal cannot dissolve in water.
Metal cannot dissolve in alcohol.

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16
Q

Simple Molecular Structure physical properties

A
  1. Low melting, boiling, points
  2. Dosen’t, conduct, electricity
  3. Dissolves, organic solvent, but not in water
  4. Soft

GILS -> sol. water
SMS -> sol. organic solvent
GMS, GIMS -> all insol.

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17
Q

DID YOU KNOW:
Pure H2o VS Graphite conductivity

A

Pure H2o has little electrical conductivity (no mobile electrons)

Graphite has high electrical conductivity (has mobile electrons)

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18
Q

Chemical Formulaes of:

Methane
Buthane
Ethanol

A

Methane: Ch4
Buthane: C4H10
Ethanol: C2H5OH

Meth: 1c
Etha: 2c
Pro: 3c
Buth: 4c
Nol: OH

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19
Q

What are allotropes?

A

Different forms, arrangments, atoms, same element

Etc allotropes of carbon
diamond and graphite

20
Q

Molecular formula
of a isotope (example) of an element

A

Formulae
Relative Molecular Mass (Given Mr in question)/Atomic Weight/Mr /relative mass of carbon

21
Q

Relative Molecular Mass

A

The bottom number in the element

22
Q

Air Mr

A

30

23
Q

Why does something not conduct electricity?

A

No, mobile, electrons, electrons are used, in ____ bonding

24
Q

Hydroxide
Carbonate
Ammonium
Sulfate
Nitrate

A

Anions
Hydroxide - OH-
Carbonate - Co3 2-
Sulfate - So4 2-
Nitrate - No3 -

Cations
Nh4 +

25
Q

Derive from the h_____ , f____ layers and m_____ e_____

Graphite properties

A
  1. High, melting, boiling, point
  2. Hexagonal, flat, layers, slide, over, easily, when, force, applied, soft, slippery
  3. High, electrical, conductivity
  4. Not soluble in organic solvent, not soluble in water

Pencil lead hates water and alcohol. Just like Diamond, and GIMS!

Unlike:
GILS - Likes water, hates alcohol
SMS - Hates alcohol, likes water

Flat and hexagonal

26
Q

Diamond properties

A
  1. High, melting, boiling, point
  2. Tetrahedral, arrangement, strong, covalent, bonds, very, hard
  3. Doesn’t, conduct electricity
  4. Doesn’t, dissolve, water, alcohol

Good friend of GMLS and lead: hates water and alcohol

Unlike GILS and SMS

GILS: Likes water, hates alcohol
SMS: Hates water, likes alcohol

27
Q

Arrangment vs Structure

A

Arrangment: Hexagonal, flat, layers, Tetrahedral Arrangment
Structure: GMS, GILS, GMLS, SMS, macromolecular

28
Q

Conductivity of Metal

A

Not all electrons are used in ____ bonding , Sea of mobile electrons, act as charge carriers

29
Q

Why are covalent bonds strong?

A

Covalent bonds result of attaction btwn positively charge atoms due to protons and shared electrons which are negatively charged, so the bonds are very strong

30
Q

Why are ionic bonds strong?

A

Electrostatic forces between positive and negative ions are very strong

31
Q

Emperical Formulae

A

formula -> proportions, elements present, not actual no., arrangment atoms

32
Q

Allotrope

A

Different, structures, formed, same, element

33
Q

When you melt or boil SMS and GMS, is it required to break strong covalent bonds?

A

GMS: Required to break strong covalent bonds
SMS: Only required to overcome weak intermolecular forces of attraction

34
Q

Valence vs Valency

A

Valence - Outer Shell
Valency - The number of electrons used to form chemical bonds

35
Q

Number of electrons used in graphite bonding

A

3/4
there is 1 free electron

36
Q

how are metal atoms held tgt in GMLS? Why are the bonds strong?

A

giant metallic lattice structure
- metal atoms held tgt strongly -> metallic bonds
- metallic bonds strong -> strong electrostatic forces between positively charged ions, mobile electrons

37
Q

what effect does metallic lattice have on electrons in GMLS?

A

giant metallic lattice structure
- atoms lose valence electrons
- mobile electrons

38
Q

how do electrons move in GMLS?

A

giant metallic lattice structure
- mobile electrons move freely in sea of electrons

39
Q

why are metals malleable and ductile?

A
  • layers, positive ions, slide over each other, take up different positions -> flexible
  • metallic bonds, not broken -> strong

recall
Malleable -> hammered into diff. shapes w/o breaking
Ductile -> drawn into wires w/o breaking

40
Q

difference betwen why metal, ionic, can conduct electricity

A

Giant Ionic Lattice Structure -> molten/aq state -> mobile ions, carry charge
Giant Metallic Lattice Structure -> mobile electrons, act as charge carriers

41
Q

physical properties of macromolecules

A
  • no fixed mp bp when formed molecules diff. sizes

REST SAME AS SMS
DOES NOT CONDUCT ELECTRICITY

42
Q

why metals have high melting, boiling pts

A
  • strong electrostatic forces requires large amt. of energy, overcome

RECALL

giant metallic lattice structure
- metallic bonds strong ->** strong electrostatic forces** between positively charged ions, mobile electron

43
Q

define alloy

A

mixture of metal w/ other elements

44
Q

physical properties of alloy as compared to pure metals

A

an alloy is…
- stronger, harder
- more resistance to corrosion

45
Q

why are alloys stronger than pure metals?

A
  • atoms from pure metal, same size, arrange in orderly manner, slide over each other easily
  • atoms from other elements, diff. size, disrupt orderly arrangement, cannot slide over each other easily
46
Q

how to draw metallic lattice

A

TAKE NOTE!!
- charges of e- must balance charges of ions
- electrons must be disorderly drawn

Chem (11 decks)

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