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MYP 4&5 Chemistry > Unit 3: How do we map matter? > Flashcards

Unit 3: How do we map matter? Flashcards

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1
Q

Atoms

A
  • Smallest unique particle
  • Nucleus + Shells
  • Neutral Charge
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2
Q

Nucleus

A

Centre of an atom

  • Protons + Neutrons
  • Positive Charge
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3
Q

Protons

A
  • Positively charged subatomic particle
  • Present in the nucleus
  • Never involved in reactions
  • Number of protons = Atomic number
  • Defines an element
  • Mass = 1
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4
Q

Neutrons

A
  • Neutral (no) charge
  • Present in the nucleus
  • Can change (isotopes)
  • Mass = 1
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5
Q

Electrons

A
  • Present in shells
  • Negative charge
  • Involved in reactions
  • Mass = 0
  • Can change (ions)
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6
Q

Anion

A
  • Negatively Charged ion

- Gained Electrons

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7
Q

Cation

A
  • Positively Charged ion

- Lost Electrons

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8
Q

Atomic Number

A
  • Number of Protons

- Defines an Element

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9
Q

Atomic Mass

A
  • Protons + Neutrons
  • Calculating Relative Atomic Mass =
    Sum of ( Abundance (%) x mass of isotope/100) for all isotopes
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10
Q

Isotope

A
  • Elements with varying number of neutrons
  • No change in protons or electrons
  • No change in charge
  • Change in mass
  • Naturally Occurring
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11
Q

Electron Shells Configuration

A

2,8,18,32 electrons per shell (spdf)

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12
Q

Metals

A
  • Give Electrons (Form anions)
  • Sonorous
  • Lustrous
  • Conductors (Heat and Electricity)
  • High Melting and Boiling Point
  • High Density
  • Ductile & Malleable
  • Opaque
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13
Q

Non Metals

A
  • Take Electrons (Form Cations)
  • Non-Sonorous
  • Dull
  • Insulators (Heat and Electricity)
  • Low Melting and Boiling Point
  • Low Density
  • Brittle - not ductile or malleable
  • Transparent(relatively)
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14
Q

Ore

A

Ores are naturally occurring rocks that contain metals or metal compounds in sufficient amounts to make it worthwhile extracting them. The method used to extract a given metal from its ore depends upon the reactivity of the metal and so how stable the ore is.
- Do not look like the metals they contain

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15
Q

Reduction of Ores using Carbon

A
  • Metals exist in ores as ‘oxides’, bonded with oxygen
  • Ores are heated with carbon
  • Carbon is oxidized, metal loses oxygen
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16
Q

Electrolysis

A
  • Ionic substances can be broken down into the elements they are made from by electricity
  • For electrolysis to work, the ions must be free to move. When an ionic compound is dissolved in water, or melts the ions break free from the ionic lattice. - Electrolyte
  • Positively charged particles go to the negative electrode (cathode) - metals are positively charged in ionic bonding
  • Negatively charged particles go to the positive electrode (anode) - non-metals are negatively charged in ionic bonding
17
Q

Reduction using Reactivity Series

A
  • Metals are arranged from most to least reactive

- More reactive metals displace lesser reactive ones in substances

18
Q

Period

A
  • Row on the periodic table
  • Elements in a period have same number of shells
  • Atomic Radius decreases as we go from left to right on a period
  • Electronegativity increases as we go left to right on a period
19
Q

Group

A
  • Columns on a periodic table
  • Elements in a group have the same valency (number of valence electrons in the outer shell)
  • Atomic Radius increases as we go up to down on a group
  • Electronegativity decreases as we go up to down on a group
20
Q

Group 1 (Alkali Metals)

A
  • Alkali Metals
  • 1 valence electron
  • Form + cations
  • Li, Na, K, Rb, Cs
  • Reactivity increases as we go down
  • React with water to form Metal Hydroxide + Hydrogen
  • More reactive displace less reactive
  • Density increases as we go down
  • Boiling + Melting point decreases as we go down
  • Very high boiling and melting points
  • Never found as elements in nature
  • Pure versions are so reactive, they are stored in oil
21
Q

Group 7 (Halogens)

A
  • Halogens (Non Metals)
  • 7 valence electrons
  • Form - anions
  • F, Cl, Br, I, At
  • Reactivity decreases as we go down
  • Displacement reactions with metals:
    MetalCl + F = MetalF + Cl
  • Density increases as we go down
  • Boiling + Melting Point increases as we go down
  • Low Boiling and Melting Pointes
  • Strong Oxidizing Agents
22
Q

Group 8 (Noble Gases)

A
  • Noble Gases (Non Metals)
  • 8/0 valence electrons
  • Odorless, Colorless
  • Stable
  • Density Increases as we go down
  • Boiling + Melting Point increases as we go down
  • Very low boiling and melting points
  • Monoatomic
  • Inert
23
Q

Transition Metals

A
  • Can have different valencies
  • Bond in metallic bonds
  • Bond in ionic bonds
  • Number of valence electrons is a roman numeral after element eg: (II)
24
Q

State Symbols

A

s, g, l, aq

  • Solid
  • Liquid
  • Gas
  • Aqueous
25
Q

Limiting Reagent

A

The limiting reagent in a chemical reaction is a reactant that is totally consumed when the chemical reaction is completed.

26
Q

Electronegativity

A
  • Increases along a period
  • Increases up a group
  • Fluorine has the highest
  • An atom’s ability to attract shared electrons to itself
27
Q

Atomic Radius

A
  • Decreases along a period
  • Increases down a group
  • Highest is Francium
28
Q

Diatomic Elements

A
  • Exist naturally as two atoms (covalently bonded)
  • 7 elements
  • non metals
  • Nitrogen
  • Hydrogen
  • Fluorine
  • Oxygen
  • Iodine
  • Chlorine
  • Bromine
    (N H F O I Cl Br)
29
Q

Polyatomic Ions

A
  • Elements bonded together that have a charge and form ionic bonds
30
Q

Galvanization

A
  • The process of applying a protective zinc coating to steel or iron, to prevent rusting
31
Q

Ionization energy

A
  • Energy required to remove an electron
  • Alkali metals - lowest
  • Increases as we move to the right (more protons in the nucleus holding electrons in)
  • Increases as we move upwards (shell is closer to the nucleus)
  • 2nd, 3rd…. ionization energies increase (more positive pull - nuclear charge), - how much energy is required to remove the 2nd, 3rd…. electron from the atom (working from outer shields inward.
  • Affected by nuclear charge, shielding electrons and distance from nucleus.
32
Q

Electron Shielding

A
  • Inner shells negative charges repel outer shells negative charges
  • Shields outermost electrons from feeling full force of nuclear charge
  • Nuclear charge - number of shielding electrons

MYP 4&5 Chemistry (7 decks)

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