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Chemistry > Unit 1: Matter, Chemical Trends and Chemical Bondings > Flashcards

Unit 1: Matter, Chemical Trends and Chemical Bondings Flashcards

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1
Q

Imagining Atoms

A
  • 2500 years ago
  • Simplest form that matter could be in, uncuttable
  • Greek meaning uncuttable
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2
Q

John Dalton

A
  • 1803
  • Law of conversation mass
  • Billard Ball Model
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3
Q

JJ Thomson

A
  • 1897
  • Electrons: negatively charged particle
  • Plum Pudding / Chocolate Chip Cookie
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4
Q

Ernest Rutherford

A
  • 1911
  • Most particles passed straight through
  • Some deflected at large angles
  • Protons
  • Nuclear Model - Gold foil experiment
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5
Q

Niels Bohr

A
  • 1913
  • Electron shells
  • Energy Levels
  • Bohr-Rutherford Model / Planetary Model
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6
Q

James Chadwick

A
  • 1932
  • neutrons
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7
Q

Erwin Schrodinger

A
  • 1926
  • Defend regions of space
  • Energy level as clouds
  • Electron Clouds
  • Quantum Mechanical Model
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8
Q

Number of electrons in each energy level

A

Energy level 1: 2 electrons
Energy level 2: 8 electrons
Energy level 3: 18 electrons
Energy level 4: 32 electrons

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9
Q

Standard Atomic Notation

A

A - mass no.
Z - atomic no. (#p & e)
X - chemical symbol
N - A-Z

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10
Q

Bohr-Rutherford diagram

A

Nucleus: proton and neutron
Orbits: electron

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11
Q

Lewis dot diagram

A

valence electrons

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12
Q

Isotopes

A

Atoms that have the same number of protons but different number of neutrons

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13
Q

Isotopes and Isotopic Abundance

A
  • Relative isotopic abundance - isotopes exist in different amounts on Earth
  • Isotopic abundance expressed in percentage
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14
Q

Determining the Atomic Mass of Elements

A

% abundance of isotope 1 (mass of isotope 1) + % abundance of isotope 2 (mass of isotope 2)

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15
Q

Radioisotopes

A
  • Repulsion between protons
  • Stabilizing - strong nuclear force
  • Radioisotopes form when n & p are not properly balanced
  • neutron decays into e & p, emits radiation and turn into different and often stable isotope
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16
Q

The development of the Periodic Table

A
  • categorized by atomic weight/mass and chemical properties
  • Dimitri Mendeleev arranged, and left empty spaces knowing there were more element
  • Henry Moseley developed method determining how many protons where in the nucleus of an atom
17
Q

Periodic Law

A

Arranged by atomic no., chemical and physical properties

18
Q

Period: row

A

Number of shells (energy level)

19
Q

Group: column

A

Valence Shell (the outermost orbit)

20
Q

Alkali Metals

A
  • Group 1
  • Soft, solid, shiny, silvery metals
  • Extremely reactive
  • Never found pure in nature
  • React with water to form bases H2
  • Reacts with halogens -> for salts
  • 1 valence electron (lose 1)
21
Q

Alkaline Earth Metals

A
  • Group 2
  • Solid, light metals
  • Never found pure in nature
  • Are reactive but less reactive than alkali metals
  • Reactive with oxygen to form oxides
  • React with water to form H2(g)
  • 2 valence electrons (loss 2)
22
Q

Transition Metals

A
  • Group 3-12
  • Very hard metals with very high melting
  • Because of their complex e configuration they can form a wide variety of compounds with other elements
  • Varies, multivalent
23
Q

Other Metals

A
  • Group 12-16
  • Not as reactive as the alkali metals or alkaline earth metals
24
Q

Metalloids

A
  • Group 13-16 (staircase)
  • Elements that have properties that are between those of metals and non-metals
    Many are shiny solids but they are poor conductors of electricity and are brittle
25
Q

Other non-metals

A
  • Group 14-16
  • Non-metals that are not H/Noble Gas
  • Not as reactive as the halogens
  • Not as unreactive
  • Most common in tissues of living things
26
Q

Halogens

A
  • Group 17
  • s, l, g / are diatomic molecules (except At
  • most reactive of the non-metals
  • Never found pure in nature
    React readily with hydrogen and other metals
  • 7 valence electrons (gain 1 electron)
27
Q

Noble Gas

A
  • Group 18
  • Colourless, odourless and unreactive
  • Stable
  • Full valence shell
28
Q

Lathanoids

A
  • Period 6 / after La
  • Rare earth metals
  • Difficult to initially separate from each other
  • Used in advanced batteries (hybrid car)
29
Q

Actinoids

A
  • Period 7 / after Ac
  • Do not have stable isotope
  • Radioactive
  • Beyond U are not naturally occuring
  • Made synthetically
30
Q

Atomic Radius

A

Distance from the center of an atom to the boundary within which the electrons spend 90% of their time

31
Q

Ionization Energy (IE)

A

Amount of energy required to REMOVE a single valence electron from an atom or ion (while in gaseous state)

32
Q

Electron Affinity (EA)

A

Energy used or released when an electron is added to a neutral atom in gas state

33
Q

Electronegativity (EN)

A

An indicator of the relative ability of an atm to attract shared electrons

Chemistry (1 decks)

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