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ch5 struct Flashcards

bonding n struct -> also include forces of attraction (55 cards)

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1
Q

Define Simple Molecular struct

A

countable no. of atoms, fixed ratio

i.e. wax molecule C18H38, know exact amt. of C,H, per molecule

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2
Q

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

A

Diamond and Silicon Dioxide:
Tetrahedral, arrangement
Giant Covalent struct
Strong covalent bonds btwn __ atoms

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

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

take note:
when asking abt strength, it is also related to amt of energy req to overcome bonds.

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3
Q

Diamond Industrial Uses

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

**Not accepted: Used as jewelry

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4
Q

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

A

Graphite: Giant Molecular Structure, many layers, carbon atoms

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

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5
Q

Desc 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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6
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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7
Q

Ionic bonds are formed by?

A

Metal, nonmetal, transferring, electrons

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8
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

any dissolved substance in water is (aq)

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9
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, rigid, withstand large forces

GMS, GMLS hates everything, does not dissolve in anything

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10
Q

Giant Metallic Lattice Structure physical properties

A
  1. High Boiling, melting, points (w/ exception, Grp 1)
  2. Good, conductor, electricity
  3. Malleable, ductile, hard
  4. Not soluble in water or organic solvent
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11
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.

PURE h2o NO electrical CONDUCTIVITY!!
it is ions that are dissolved in h2o i.e. Na+ ions in tap water, that causes conductivity

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12
Q

What are allotropes?

A

Different forms, structural arrangments, atoms, same element

Etc allotropes of carbon
diamond and graphite

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13
Q

Molecular formula
of a isotope of an element

A

Relative Molecular Mass (Given Mr in question)/Mr according to periodic table

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14
Q

Air Mr

A

30

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15
Q

Phosphate

A

Po4 3-

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16
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, small amt energy break struct apart
  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

graphite layers easy to separate

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17
Q

Diamond properties

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

GMLS, Lead, Diamond: hates water and alcohol

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

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18
Q

Arrangment vs Structure

A

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

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19
Q

Conductivity of ??except metal format

A

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

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20
Q

Why are ionic bonds strong?

A

Electrostatic forces between positive and negative ions are very strong

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21
Q

Emperical Formulae

A

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

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22
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

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23
Q

Valence vs Valency

Study These Flashcards
A

Valence - Outer Shell
Valency - no of outer shell electrons

24
Q

Number of electrons used in graphite bonding

graphite 1 carbon bond to __ carbon

Study These Flashcards
A

3 electrons used, 1 free electron

1 carbon bond to 3 other carbon

25
how are metal atoms held tgt in GMLS? Why are the bonds strong?
- metal atoms held tgt **strongly** by metallic bonds - metallic bonds **strong** -> strong electrostatic forces between **positively charged ions**, mobile electrons ## Footnote giant metallic lattice structure
26
what effect does metallic lattice have on electrons in GMLS?
giant metallic lattice structure - atoms lose valence electrons - mobile electrons
27
how do electrons move in GMLS?
giant metallic lattice structure - mobile electrons move freely in sea of electrons
28
why are metals malleable and ductile?
- layers, positive ions, slide over each other, **take up different positions** -> flexible - metallic bonds, not broken -> strong ## Footnote **recall** Malleable -> hammered into diff. shapes w/o breaking Ductile -> drawn into wires w/o breaking
29
difference betwen why metal, ionic, can conduct electricity
**Giant Ionic Lattice Structure** -> molten/aq state -> mobile **ions**, carry charge **Giant Metallic Lattice Structure** -> mobile **electrons**, act as charge carriers
30
define alloy
mixture of metal w/ one/more other elements
31
physical properties of alloy as compared to pure metals
**an alloy is...** - stronger, harder - more resistance to corrosion - less malleable, ductile than pure metals - melt over range, temp, mixture ## Footnote metal, alloy both good conductor of heat
32
why are alloys stronger than pure metals?
- **pure metal** atoms, same size, arrange orderly manner, slide over each other easily - atoms from other elements, diff. size, disrupt orderly arrangement, cannot slide over each other easily ## Footnote ALLOYS HAVE IRREGULAR LATTICE ARRANGEMENT
33
how to draw metallic lattice
**TAKE NOTE!!** - charges of e- must balance charges of ions - electrons must be disorderly drawn
34
4 example of alloys + what they contain
1. brass (Cu, Zn) 2. bronze (Cu, Sn) 3. steel (Fe, C) 4. Stainless steel (Fe, C, Ni/Cr) -> **slower rusting**
35
macromolecular properties
1. covalent substances, i.e. polymers 2. insoluble in water, soluble, organic solvent 3. no fixed mp, bp when formed, molecules, diff sizes, **soften over range, temp, when weak intermolecular FoA overcome** 4. do not conduct electricity
36
what are metallic bonds
strong electrostatic force, attraction btwn sea of mobile e-, positive ions
37
why metal high mp, bp
1. strong electrostatic force, attraction btwn sea of mobile e-, positive ion 2. form, giant metallic lattice struct, 3. struct requires large amt energy, overcome
38
why metal does not dissolve in organic solvent/water?
strong electrostatic forces of attraction btwn positively charged metal ions, sea of mobile electrons too strong, broken by solvent
39
why GILS hard but brittle
hard -> strong electrostatic forces of attraction, btwn opposite charged, ions brittle -> force applied, shift ions, lattice positions, repulsive force, btwn ions, same charge strong enf overcome electrostatic forces of attraction, cause loss, lattice struct
40
why GILS more charge, melting pt higher
bigger charge, ions stronger electrostatic forces of attraction more heat energy req overcome ## Footnote i.e. Mg2+ and O 2- > Na+ and Cl- forces of attraction
41
why GILS cannot conduct electricity, solid
held tgt, fixed positions, lattice struct in solid state no mobile ions
42
why __ struct is transparent
single layer of atoms, very **thin**
43
giant ionic lattice struct why can dissolve, water
strong attraction, polar water molecules charged ions, ionic compound
44
sms why can dissolve, organic solvent
simple molecular struct non polar organic solvents non polar ## Footnote 1. polarity: which means charge or non charge. 2. water polar. organic solvent non polar. like dissolves like. 3. too strong to be broken by solvent (hence gms, gmls no dissolve)
45
methods of chemical separation
- thermal decomposition - electrolysis
46
graphite funct
pencil lead, solid lubricant ## Footnote pressing pencil lead on paper, shear away layers, graphite
47
example of polymer with low mp, bp
poly(ethene)
48
valency in covalent bonding
no. of electrons shared in order ion attain stable config
49
chemical species
an atom/ion ## Footnote using the same method to determine O.S., can determine charge of individual element in a compound
50
(aq) need to be ionic substance that dissociate
anything dissolved in water (i.e. I2 (aq) - covalent substance) ## Footnote such substances dun need split into ions when dissolve in water
51
spectator ion definition
ions, does not take part, reaction, remain unchanged, phys state
52
phys properties chem properties KMno4 oxidise, KI reduce is always redox?
**phys** - odor - mass, vol - density - viscos - sol - pH - flammability **chem** - how it react - i.e. redox react w/ KMno4/KI ## Footnote **KMno4 oxidise, KI reduce is always redox?** Yes.
53
precipitation vs displacement
**displacement:** more reactive metal/halogen displace metal salt/halide **ppt.**: sol salt + sol salt -> insol salt + sol salt
54
carbonate alkali?
all g1 carbonate alkali dissolve form OH- ions in soln.
55
what dissolve in organic solvent
as long as got C, H mostly dissolve in organic solvent
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