C2.2 Flashcards

1
Q

Metals properties what is ductile and malleable

Lustrous

A

Metals shiny high melting boiling, malleable *THEY BEND WITHIUT SHATTERING) Ductile (they can Be PULLED INTI WIRES) conductors.

HIGH DENSITIES
LUSTROUS (SHINY)

Non metal dull low gas solid, brittle, not ductile insulators.

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2
Q

How is periodic table arranged

A

Row colum, increasing atomic number

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3
Q

What happens when metal oxide vs non metal oxide dissolve in water?

A

Alkaline for metal (sodium oh)

Acidic for non metal

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4
Q

Electronic structure relations

What are max electrons per shell

A

This just 2.8.8

Number of numbers = periods
Sum is atomic
Last is group non iupac

Max is 2.8.8.2

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5
Q

Joined compunds properties

A

1) Have strong forces of electrostatic forces between them
2) from giant ionic lattices, closely packed REGULAR LATTICE
3)
- since string force , high boiling melting point
- can’t conduct electricity solid, but dissolved in water or Moneten it can because charged particles are free to carry charge
- dissolve easily in water

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6
Q

Ball and stick diagram for ionic compounds advantage disadvantage

A

Good for showing how ions arranged but bad scale as nit that close too each other real life. Ions closer too each other and bonds are actually FORCES NOT BONDS.

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7
Q

Covalent properties

Dot cross

A

Non metal only
Valence shell shown only.
Covalent form simple molecular structures (like water), a simple molecule contains a few atoms

1) covalent binds are strong forces of electrostatic attraction between shared pair of electrons and the nucleus. However in simple molecular it’s intermolecular which is weak and easily over come therefore low boiling melting.

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8
Q

Ball ans stick model advantage disadvantage for covalent..

A

Good as it shows three dimensional structure of model, and makes it easier to understand

Bad because size of atoms and length of bonds exaggerated and suggests electrons that make the bonds don’t move but rather fixed

Displayed formula good but not 3D..

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9
Q

Giant covalent carbon allotropes

GRAPHENE? What is it and what advantages

Fullerenes ( or giant)
Formula for buckministerfullerene
What is shapes of Bucky ball and what are they used for

A

Lot of non metal covalently bonded. Formula given empirical so diamond just C.

  • highnboiling pointe
  • don’t conduct electricity except for graphite

Diamond

  • carbon form 4 bonds rigid covalent structure, making it hard
  • good cutting tools high boiling too no electricity

Graphite
Carbon for, 3 covalent bonds, creating sheets of carbon layers that are free to slide over (so pencil) layers slippery so rubbed off for marks
- the other outer electrons are delocalised and free to move, this means conduct electricity
- high boiling
-SINGLE SHEET OF GROWHITE CALLED GRAPHENE. Very good, conduct better, thin and transparent and LIGHT.

Fullerenes

  • made up of carbon molecules, not GIANT COVALENT
  • intermolecular so lower boiling points, but decently high for that cause lot of intermolecular still
  • delocalised electricity
  • Rings arranged, hollow inside
  • BUCKY BALL IS USED AS LUBRICANTS, and molecules act like tiny ball bearings, with pentagons and hexagons. Can transfer medical drugs directly to cells

4) c60

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10
Q

Polymers

Thermosetting
Thermosoftening

Which can be remoulded?

A

Repeating units monomers held together by COVALENT bonds

  • REpresnted by curvy lines
  • usually alkenes and carbon based
  • all held by covalent in chains, but across the chains if intermolecular holds them together, then weak therefor themrmosftening, if covalent are used called cross links then thermosetting. Sometimes intermolecular held across which are stronger…
  • thermosetting is high boiling and rigid, can’t be stretched
  • thermosoftening free TO SLIDE IVER EAVH OTHER, STRETCHED SND LOW BOILING

1) thermosoftening because bonds weak

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11
Q

Metallic properties

A

All metal solid except MERCURY

Form string electrostatic forces of attraction between positive metal ion and negative delocalised electrons , giving high melting boiling etc

1) this makes the form GIANT METALLIC LATTCIES, regular, touching

A sea of delocalised electrons form when electrons leave valence shells of metal

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12
Q

Advantage disadvantage if modelling metallic

A

Metallic is lattice is extends in 3D directions.

Lose Info when you do 2d

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13
Q

How big are nano particles

What are fullerenes (in terms of nano:

What re the properties of nano and why used (catalysts, sun creams, medicine, sports, antibacterial) paints

Disadvantage of nanoparticles?

A

1- 100nm long

2) bigger then atoms by 100
3) FULLERENES are Nano particles
4) high SA:V, therefore very useful for CATALYSTS
5) don’t leave marks in sun creams and deodarsnsts, do job
6) nano medicine, as they are absorbed easily by body, they can DELIVER DRUGS WHERE THEY NEED TO

7) conduct electricity, so are used in ELECTRIC CIRCUITS
8) added to plastics in sport like racket, make them stringer and durable without adding much mass
9j) Silver nanoparrifles give ANTIBACTERIAL PROPERTIES
10) good for Paints

1) SCIENITSIST DINT FUKLY UNDERSTAND THE EFFECT IF NANOPARTICLES ON HUMANS, there may be side effects in the long term, they easily breathed in or go to cells, and because TOXIC SUBSTANCES MAY GO IN THEM, them taking a long time to break down,..

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14
Q

How did Mendeleev arrange the elements of the periodic table in 1869

A

1) he arrange them in order of ATOMIC MASS, and the similar chemical properties.
- to do so, he had to leave some GAPS where he thought elements with those similar chemical properties would fit but just not discovered yet.
- had to swap around a few elements, such as tellurium and Idolen to better fit the properties

2) ARRANGED IN ROWS, not columns
3) by 1871 he rotated it, making it groups and rows
4) his predictions , such as that if germanium, came true, proving he was right, and fitted in empty spaces

5) then MOSELY discovered the number if protons was the atomic number, and this PROVED MENDELEEV right in his theory about swapping iodine and tellurium around.

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15
Q

What happens next (as in how did group 0 come)

Now?

A

Lord Rayleigh and William Ramsay discovered argon on 1894

  • even Mendeleev didn’t think this was possible, because he though all element should react with each other
    2) then helium discovered. The n krypton and neon.
    3) Ramsay suggested to make new group- he did

1) increasing atomic number, electronic structure determines chemical properties,

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16
Q

WHAT ARE ALLOTROPES

Example for carbon

A

Different forms of an element in different atomic arrangements

Such as diamond and groahite allotropes of carbon

17
Q

How does something melt

Solid to gas

Gas to solid

A

When thermal energy is provided, particles gain energy in kinetic stires, moving more, eventually having enough energy to overcome bonds, and change state.

Sublimation is when solid to gas
Deposition is gas to solid

18
Q

Bulk properties of 3 substances and why?

Brittle or no

A

Metals= can slide over each other to become malleable because when the particles move a bit left due to large force, and there are delocalised electrons, the bonds don’t actually break, so it’s fine

Giant covalent however when large enough force is applied a lot of covalent bonds are broken at once, causing it to break. Similar YB happens in giant ionic, this makes it BRITTLE.

Simple molecular/ ploymers= are brittle in solid form and lattice form, but if NOT LATTICE FORM THEN THEY CAN BE FLEXIABLE AND SOFT

19
Q

Why use to cover paper

A

Quicker
Sensitive do smaller sample used

More stationary and mobile to chose from