ch5 struct

Question 1

3 types of bonding

Answer 1

Covalent, Metallic, Ionic

Question 2

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

Answer 2

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

Question 3

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

Answer 3

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.

Question 4

Diamond Industrial Uses

Answer 4

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

**Not accepted: Used as jewelry

Question 5

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

Answer 5

Graphite

Question 6

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

Answer 6

Graphite: Giant Molecular Structure, many layers, carbon atoms

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

Question 7

Desc Graphite forces and bonding

Answer 7

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

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

Question 8

cube

Giant Ionic Lattice Structure forces and bonds and structure

Answer 8

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

Question 9

Ionic bonds are formed by?

Answer 9

Metal, nonmetal, transferring, electrons

Question 10

Derive

Giant Ionic Lattice Structure - Physical Properties

Answer 10

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

Question 11

Giant Molecular Structure physical properties

Answer 11

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

Question 12

Giant Metallic Lattice Structure physical properties

Answer 12

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

Question 13

Simple Molecular Structure physical properties

Answer 13

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

Question 14

What are allotropes?

Answer 14

Different forms, arrangments, atoms, same element

Etc allotropes of carbon
diamond and graphite

Question 15

Molecular formula
of a isotope of an element

Answer 15

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

Question 16

Air Mr

Answer 16

30

Question 17

Phosphate

Answer 17

Po4 3-

Question 18

Derive from the h_____ , f____ layers and m_____ e_____

Graphite properties

Answer 18

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

Question 19

Diamond properties

Answer 19

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

Question 20

Arrangment vs Structure

Answer 20

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

Question 21

Conductivity of ??except metal format

Answer 21

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

Question 22

Why are ionic bonds strong?

Answer 22

Electrostatic forces between positive and negative ions are very strong

Question 23

Emperical Formulae

Answer 23

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

Question 24

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

Answer 24

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

Question 25

Valence vs Valency

Answer 25

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

Question 26

Number of electrons used in graphite bonding graphite 1 carbon bond to __ carbon

Answer 26

3 electrons used, 1 free electron 1 carbon bond to 3 other carbon

Question 27

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

Answer 27

- 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

Question 28

what effect does metallic lattice have on electrons in GMLS?

Answer 28

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

Question 29

how do electrons move in GMLS?

Answer 29

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

Question 30

why are metals malleable and ductile?

Answer 30

- 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

Question 31

difference betwen why metal, ionic, can conduct electricity

Answer 31

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

Question 32

physical properties of macromolecules

Answer 32

- no fixed mp bp when formed molecules diff. sizes ## Footnote **REST SAME AS SMS** **DOES NOT CONDUCT ELECTRICITY**

Question 33

define alloy

Answer 33

mixture of metal w/ one/more other elements

Question 34

physical properties of alloy as compared to pure metals

Answer 34

**an alloy is...** - stronger, harder - more resistance to corrosion

Question 35

why are alloys stronger than pure metals?

Answer 35

- **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

Question 36

how to draw metallic lattice

Answer 36

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

Question 37

4 example of alloys + what they contain

Answer 37

1. brass (Cu, Zn) 2. bronze (Cu, Sn) 3. steel (Fe, C) 4. Stainless steel (Fe, C, Ni/Cr) -> **slower rusting**

Question 38

macromolecular struct

Answer 38

1. covalent substances, i.e. polymers 2. insoluble in water, soluble, organic solvent 3. no fixed mp, bp when formed, molecules, diff sizes 4. **some polymers i.e. polyethene low mp, bp** -> weak intermolecular forces of attraction, molecules 5. do not conduct electricity

Question 39

what are metallic bonds

Answer 39

strong electrostatic force, attraction btwn sea of mobile e-, positive ions

Question 40

why metal high mp, bp

Answer 40

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

Question 41

why metal does not dissolve in organic solvent/water?

Answer 41

strong electrostatic forces of attraction btwn positively charged metal ions, sea of mobile electrons too strong, broken by solvent

Question 42

why GILS hard but brittle

Answer 42

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

Question 43

why GILS more charge, melting pt higher

Answer 43

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

Question 44

why GILS cannot conduct electricity, solid

Answer 44

held tgt, fixed positions, lattice struct in solid state no mobile ions

Question 45

why __ struct is transparent

Answer 45

single layer of atoms, very **thin**

Question 46

giant ionic lattice struct why can dissolve, water

Answer 46

strong attraction, polar water molecules charged ions, ionic compound

Question 47

sms why can dissolve, organic solvent

Answer 47

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)

Question 48

elements from period ___ on no need follow rule, 8 valence e-

Answer 48

period 3 2n^2 also works to check this out. ## Footnote check this if drawing involve greater than period 3 element