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Chem definitions > 1, 2, 3 for test 1 > Flashcards

1, 2, 3 for test 1 Flashcards

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1
Q

Molar mass measured in vs atom

A

g/mol is molar mass as you can measure it yourself. A singular atom is measured in amu as it is very small

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2
Q

Bohr’s model

A

Full electron diagram for atom showing protons, neutrons and electrons and energy shells

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3
Q

Cations

A

Metal ions, want to loose electrons. Have a low first ionisation energy, loose electrons to become positive.

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4
Q

First Ionisation energy

A

energy required to remove the outer most electron from an atom.

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5
Q

Group on the periodic table - dictate

A

Vertical columns that indicate how many electrons are in the valance shell of atoms.

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6
Q

Period number of an element

A

Rows on the periodic table. Tells us how many electron shells atoms have.

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7
Q

Atomic radius

A

Distance between the nucleus and the valance shell.

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8
Q

Electronegativity

A

Ability of an atom to attract electrons.

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9
Q

Down a group atomic radius

A
  • atomic radius increases as more electron shells
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10
Q

Electrostatic attraction

A

Force of attraction between electrically charged particles due to their opposite charges

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11
Q

Across a period atomic radius

A
  • Atomic radius decreases as more proteins means stronger charge of nucleus that pulls electrons in tighter
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12
Q

Across a period 1st IE

A
  • 1st IE increases as it is harder to loose e as the nuclear charge is acting over a shorter distance so energy required to remove an e increases
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13
Q

Across a period electronegativity

A
  • increases excluding group 18 as the nuclear charge increases as more protons in nucleus so increased attraction to electrons
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14
Q

Down a group 1st IE

A
  • 1st IE decreases as decrease in electrostatic attraction
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15
Q

Down a group electronegativity

A
  • decreases as the atomic radius increases so decrease in electrostatic attraction so less attraction to electrons
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16
Q
A
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17
Q

Reactivity - position on period table

A

Elements that are more reactive gain/loose electrons more easily to have a stable electron configuration. Non metals in group 17 and metals in group 1 and 2.

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18
Q

Properties of elements in the same group

A

Same number valence e, same charged ions, same bonding capability

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19
Q

Properties of elements in the same period

A

Same number of electron shells

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20
Q

Isotopes definition

A

Atoms of the same element (same number of protons) but differing numbers of neutrons. C-12, C-13, C-14

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21
Q

Isotope properties

A

Same chemical properties (reactivity and charge of ions) but different physical properties (density, mass and melting point)

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22
Q

Same chemical properties

A

same chemical properties react similarly in chemical reactions. Atoms in the same group have same chemical properties.

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23
Q

Same physical properties

A

same physical properties exhibit similar characteristics related to their physical state or appearance or mpt/bpt

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24
Q

Mass spec

A

Separates isotopes based on their mass. It is a technique that identifies which isotopes are present as well as their abundance. Determines the relative atomic mass of elements.

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25
Q

Relative atomic mass measures in

A

measured in amu. Atomic mass units.

26
Q

Calculate relative atomic mass - equation

A

RAM = %1 x M1 + %2 x M2
etc

27
Q

Stoich ratio equation

A

N unknown = u/k x nknown

28
Q

Percentage by mass calculation (carbon)

A

%c = mass C/mass CO2 x 100

29
Q

Transition metals

A

Have to specify their charge

30
Q

ide

A

Non metal element as an ion

31
Q

ate

A

Polyatomic ion with maximum amount of oxygens it can handle

32
Q

ite

A

element with 1 less oxygen than ates

33
Q

Conductivity

A

Ability to conduct electricity, allowing the flow of an electric current, mobility of charge carriers (electrons or ions)

34
Q

Ionic bonds
electron distribution, physical properties and conductive properties

A
  • Cations loose e and Anions gain, form a lattice structure of pos and neg charged ions
  • Very high mpt/bpt, crystal lattice structure is brittle
  • Not conductive as solid
  • Conductive as liquid or aqueous as mobile ions carry charge
35
Q

Covalent molecule
electron distribution, physical properties and conductive properties

A
  • Electrons are shared between atoms, not always shared equally which makes the molecule polarized
  • low mpt/bpt, usually gases at room temperature, share e
  • cannot conduct electricity as no mobile charged particles
36
Q

Covalent network
electron distribution, physical properties and conductive properties

A
  • electrons are shared in an ‘infinite network’
  • V.V.V high mpt/bpt, brittle
  • Diamond and glass cannot conduct electricity but graphite can
37
Q

Why graphite is conductive

A

Each carbon atom is covalently bonded to three other carbon atoms the arrangement leaves one electron per carbon atom uninvolved in bonding resulting in delocalized electrons within the layers of graphite. Mobile charged elections facilitate conductivity.

38
Q

Order of bonding types in mpt/bpt

A

Covalent network, Ionic, metallic, Covalent molecule

39
Q

polyatomic ions

A

2 or more atoms bonded together with net charge

40
Q

Avogadro’s number

A

6.022 x 10^23 particles

41
Q

Law of conservation of mass

A

Mass is neither created nor destroyed in a chemical reaction. The total mass of the reactants must equal the total mass of the products in a chemical equation.

42
Q

Electrostatic attraction in metallic bonding

A

Electrostatic forces between nuclei of atoms to their delocalized electrons

43
Q

Electrostatic attraction in covalent molecular bonding

A

Strong intramolecular forces between positive nuclei and shared electrons

44
Q

Intramolecular forces in covalent network

A

Strong intramolecular forces throughout the structure, between positive nuclei and shared electrons. Significant energy is required to break these bonds.

45
Q

Ionic bonds are brittle

A

When alignment shifts the similar charges repel and the lattice breaks

46
Q

Intermolecular forces

A

force of attraction between neighbouring molecules

47
Q

Reactivity

A

Measure of how readily a substance interacts with other substances to form new chemical bonds and undergo chemical transformations.

48
Q

Covalent network structure

A

lattice of atoms bonded together by covalent bonds in an ‘infinite structure’.
Glass and carbon are Very hard and rigid structure from tightly packed atoms makes structure brittle.

49
Q

Allotrope

A

Different structural form of the same element. Allotropes of carbon are diamond and graphite.`

50
Q

Cdiamond

A

Each carbon bonded to 4 other carbons, not conductive as no free mobile charge

51
Q

Cgraphite

A

Each carbon bonded to three other carbons, 1 spare electrons means graphite is conductive.`

52
Q

Nanotechnology

A

Manipulation of matter at nanoscale, at this scale materials exhibit different properties to bulk materials as of high SA/Vol ratio.

53
Q

Nanoparticles

A

Very small structures between 1 and 100 nanometres in size

54
Q

Examples and use of a nonotechnology

A

Nano silver has antibiotic and fungal properties

55
Q

Stumbling blocks for the development of nano technology

A

Not understood the health and environmental risks. If put nano silver into sports clothing could have bad affects on environment when washed.

56
Q

Isotope properties

A

Came chem properties, different physical properties

57
Q

Electron config vs bohrs model

A

Config = listing electrons in electron shells (2,4)
Bohrs model shows the number of shells, electrons, protons and neutrons

58
Q

Observations for partial dissolving - excess solid reactant

A

xx produce xx and some silver granules remain

59
Q

metallic bonds
electron distribution, physical properties and conductive properties

A
  • delocalised sea of electrons
  • high mpt/bpt, lusterous, sea of electrons, malleable
  • V.V good conductivity, delocalised electrons allow current to flow
60
Q

electrostatic attraction in ionic bonding

A

Strong electrostatic forces between positive ion and negative ion in the crystalline lattice. High electrostatic attraction contributes to high mpt/bpt

Chem definitions (8 decks)

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