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Chemistry Unit 1 > Topic 1 - Data test > Flashcards

Topic 1 - Data test Flashcards

1
Q

What is the Aufbau Principle

A

Electrons enter orbitals at the lowest energy first (fill lowest first)

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2
Q

What principle is when ‘Electrons enter orbitals at the lowest energy first (fill lowest first)’

A

Aufbau Principle

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3
Q

What is Pauli exclusion principle

A

no pair of electrons in an atom can have the same quantam numbers

  • atomic orbital may descirbe at most 2 electrons
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4
Q

What principle is when
“no pair of electrons in an atom can have the same quantam numbers - atomic orbital may descirbe at most 2 electrons”

A

Pauli exclusion principle

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5
Q

What is Hund’s Rule

A

When electron occupy orbitals of equal energy levels –> one electron enters each orbital until all oribitals contain one electron

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6
Q

What rule ‘When electron occupy orbitals of equal energy levels –> one electron enters each orbital until all oribitals contain one electron’

A

Hund’s Rule

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7
Q

State electron confiuration until 4d10

A

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10

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8
Q

Metal + H20 (water) –>

A

Metal Hyrdoxide + H2 gas

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9
Q

Metal + Oxygen –>

A

metal oxide

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10
Q

Metal + Acid –>

A

Salt + H2 gas

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11
Q

What is electron config of a K+ ion

A

1s2 2s2 2p6 3s2 3p6

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12
Q

What is positive nuclear charge

A

Caused by protons (charge from protons on electrons) that pull electrons closer and increase ionization energy

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13
Q

What is shielding effect

A

Caused by electon shells shielding valence electron from positive nuclear charge and thus decreased charge and decreasing ionization energy

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14
Q

Positive nuclear charge and shielding effect left-right period and down group

A

atomic number increases poeriod - more protons acting on each other - thus eletrons closer to protons since higher positive nuclear charge of more protons on each electron

shielding effect increases down a group since the previous shells shield the positive nuclear charge on valence electrons, requireing less ionization energy - to remove electrons

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15
Q

How does the radius of atoms change due to what ion it is

A

Less radius of cations since less electrons and protons (+ve nuclear charge) can act on electrons more efficientley (1 less electron for unchanged protons to attarct closer) and opposite with anions
- Repulsion is larger with more electrons also pulling electrons further away from nucleas increasing radius
(anions = bigger radius)
(cations = smaller radius)

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16
Q

What is ionization energy

A

The minimum energy that is required to remove an electron from the outermost shell of an atom in it’s gaseous state

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17
Q

How to write the first ionization energy of (Na)

A

Na(g) –> Na+(g) = e-(g)

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18
Q

What is the trend of ionization energy across a period from left to right

A

Left to right a period - n. protons increase - +ve nuclear charge increases –> valence electrons are pulled closer to the nucleas thus is harder to remove and

(INCREASE IN IONIZATION ENERGY)
with 4 exceptions each period

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19
Q

What is the trend of ionization energy down a group

A

N. shells increases –> +ve nuclear charge is blocked due to the shielding effect since protons have less attraction to the valence electrons + repulsion of valence electrons pushing them outward makes it easier to remove valence electrons

(DECREASE IN IONIZATION ENERGY)

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20
Q

Explain the exception in ionization energy across left to right period (that it should increase left to right)

A

(only up to period 4) Between group 2 and 13 –> 2

Group 2 has full electron subshell of s2 therfore it takes more energy to remove from more stable electron config
Group 3 has one extra in p1 and wants to lose it to gain a more stable full subsheel of s2 thus less energery is required to remove it

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21
Q

What is electron affinity?

A

How easy it is to accept electrons into a gaseous state atom into a anion (higher easier to accept electrons) and vise versa

the amount of energy released when an electron attaches to a neutral atom or molecule in the gaseous state to form an anion

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22
Q

What is electronegativity?

A

The ability an atom has to pull electrons towards itself
Defines how likely an atom can form a cation/anion

  • since LOW ionization energy & LOW affinity = pull electron away = cation
  • HIGH ionization energy & LOW affinity = pull electron towards = anion
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23
Q

What oxides do non-metals generally form

A

Non-metals can dissolve in water to form acidic oxides

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24
Q

What oxides do metals generally form

A

Metals can dissolve in water to form basic oxides (alkaline solutions)

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25
Q

What happans to amphoteric metal oxides

A

React with both acids and bases to create salts and water

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26
Q

How does Sulfer and O2 react in water and where does it come from

A

Sulfer and Dioxide –> Sulphur Dioxide + Water –> acidic rain

sulfer is gained from coal burning

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27
Q

How do oxides change from left to right a period and down a group

A

Oxides go from basic –> amphoteric –> acidic
More electronegativity = more acidic it is

DOWN -
increases in basic down a group since electronegativity generally decreases (with transition metals vary)

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28
Q

What are three acidic oxides to memorise

A

CO2 - Carbon Dioxide
SO2 - Sulfur Dioxide
NO2 - Nitrogen Dioxide

All form acids/acid rain when react with water and oyxgen in air

Add 2 hydrogen at front and an extra oxygen (CO2 –> H2CO3 or H2CO2 (can vary between 2/4 or 3 but 2 is usually the acid rain)) (Carbonate acid)

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29
Q

What happans when Nitrogen Oxide reacts with water and where does it come from

A

Cars produce nitrogen –> acid rain since caues HNO2 or HNO3 and falls

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30
Q

What is H2SO4 or H2SO3

A

H2SO4 = Sulfuric acid
H2SO3 = sulfourius acid

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31
Q

What are all the properties of ionic bonds
- electricity
- structure
- force
- physical property
- Between…

A
  • Crystal lattice structure of a 3 dimensional arrangement of positive and negative ions
  • Conduct electricity if dissolved in solvent since electrons are free to move - solid cannot
  • Electrostatic force of attraction between oppositely charged (+ve and -ve) ions
  • Hard and brittle
  • Metal + Non-metal
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32
Q

What are all the properties of covalent bonds
- electricity
- structure
- force
- physical property
- Between…

A
  • There are simple molecular covalent e.x.(NH3, H2O, CH4)
  • Between non-metals (no ions)
  • The sharing of electrons
  • There are no free electrons thus cannot conduct electricity
  • Electron clouds overlap and both protons attract electron to share it
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33
Q

Acids and bases with electricity?

A

Strong acids + bases are good conductors and thus good electrolytes

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34
Q

Define valency

A

The power to combine

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35
Q

How strong are ionic vs covalent bonds

A

Ionic bonds are stronger than covalent since harder to break covalent

36
Q

What is the molecular and electronic geomtery + angle of Methane

A

CH4 - tetrahedral in molecular - tetrahedral in electron geometry
109 degrees

37
Q

What is methane

A

CH4

38
Q

What is ammonia

A

NH3

39
Q

What is ammonium

A

NH4

40
Q

What is the molecular and electronic geomtery + angle of Water

A

H2O - Bent molecular - tetrahedral electron
104.5 degrees

41
Q

What is the molecular and electronic geomtery + angle of Ammonia

A

NH3 - Pyramidal molecular - tetrahedral electronic
107 degrees

42
Q

What is it called when a liquid dissolves into a liquid

A

Miscible

43
Q

What is it called when a solid dissolves into a liquid

A

Soluble

44
Q

The 3 chemical compounds that are so strong they cant dissolve in water

A

CaCO3
AgCl
BaSO4
Insoluble in water since the bonds are so strong there is not enough energy in the water

45
Q

What are physical properties

A

observed without a chemical change/changing identity of a substance (melting points, density, malleability, boiling point)

46
Q

What are chemical properties and example

A

(flammability, corrosion, oxidation, PH, reactivity) - how a substance changes into a different cubstance

47
Q

Patterns of Halogens

A

Reactivity decreases down, MP,/BP increase down, Density increase down

48
Q

Patterns of alkali metals

A

Reactivity increases down, MP,BP decrease down, Density increase down, soft, shiny and silver colour

49
Q

What is the pop test

A

Hydrogen gas test by adding flint to h2 and u get a pop

50
Q

List all diatomic gases, how many are there?

A

7 –> H, N, O, F, Cl, Br, I
Have no fear of ice cold bear

51
Q

What is direct synthesis combination?

A

2/more substancces react together to form 1 product (A + B –> AB)

52
Q

What is a single replacement reaction?

A

When a more reactive element displaces a less reactive one from a solution of one of it’s compound and switches

(AB+C –> AC + B)

Look at reacitivty, if the single is more reactive than the other metal, it will replace

53
Q

What is combustion?

A

Always has a Hydro-carbon (Carbon and hydrogen) e.x. CH4 AND oxygen as reactants to create carbon dioxidxe and water - becoming a exothermic reaction (fire/heat/explosion)
C3H8 + O2 –> CO2 + H2O
CH4 + O2 –> CO2 + H2O
(can have a oxygen in the hydrocarbon)

54
Q

What is a suspension

A

Heterogeneous mixture of a fluid that contains solid particles sufficiently large for sedimentation

55
Q

What is an alloy

A

Metal made by combining two or more metallic elements, especially to give greater strength or resistance to corrosion - will have properties of a metal

56
Q

What is a solvent in relation to solute

A

The substance in which a solute dissolves to produce a homogeneous mixture

57
Q

What is a solute

A

Something that gets dissolved in a solvent like salt or sugar

58
Q

What is a

A

Something composed of two or more separate elements; a mixture

59
Q

What is a molecule

A

Two or more atoms held together by bonds

60
Q

Describe the properties of sodium chloride

A
  • 3D dimensional arrangement of +ve & -ve ions (neg Cl and pos Na)
61
Q

Whats the relationship between polarity and electronegativity

A

The bigger the electronegativity difference the higher polarity

62
Q

What is isoelectronic

A

Having the same numbers of electrons or the same electronic structure
E.x. N3- and Ne and Na+ all have same electorn count

63
Q

What is isoelectronic

A

Having the same numbers of electrons or the same electronic structure
E.x. N3- and Ne and Na+ all have same electorn count

64
Q

What is an allotrope

A

Each of two or more different physical forms in which an element can exist. Graphite, charcoal, and diamond are all allotropes of carbon.

65
Q

Why is the second ionization energy always higher than the first

A

The second ionization energy is always larger than the first ionization energy, since it requires even more energy to remove an electron from a cation than it is from a neutral atom

More protons vs electrons + less repulsion so would pull closer

66
Q

What is decomposoiton reaction?

A

A compound that is broken down into simpler compounds, or all the waydown to the elements that make it up
H2O –> H2 + O
AB –> A + B
CaCO3 –> CaO + CO2

67
Q

What is a double replacement reaction?

A

(AB + CD –> AC + BD)
The positive and negative ions in two compounds switch places
BaCl2 + NaSO4 –> BaSO4 + NaCl

68
Q

What is a redox/oxidation-reduction reaction?

A

Reduction –> gain of electrons
Oxidation –> loss of electrons

Na –> Na + e- Oxidation
Cl + e- –> Cl- Reduction
^ these 2 are called half reactions

Na + Cl –> Na+Cl-

69
Q

What indicates a chemical reaction

A

Release of energy as heat
Release of energy as light
Formation of gas
Change in colour
Chnage in odour

70
Q

What is a neautralization reaction?

A

Acid + base –> salt + water
H + OH –> H(OH)

HX + MOH –> MX + H2O
Where X/M are elements

Neutralization reactions occur when an acid (most compounds starting with H) and a base (most compounds ending in OH) react to form a salt and water
- A type of double replacement

70
Q

What is a neautralization reaction?

A

Acid + base –> salt + water
H + OH –> H(OH)

HX + MOH –> MX + H2O
Where X/M are elements

Neutralization reactions occur when an acid (most compounds starting with H) and a base (most compounds ending in OH) react to form a salt and water
- A type of double replacement

71
Q

What is the reactiivyt of elements in periodic table

A

Metals –> more to left and down = highest
Non metals –> more to the right and top = highest (disregarding noble gases and metataloids)

72
Q

What are all reactions

A

Synthesis
Decomposition
Double Replacement
Single replacement
Redox
Neutralization
Combustion

73
Q

Differnet Ph levels and their meanings

A

7 = neautral
8 to 14 = base
6 to 0 = acid

74
Q

, Why does reactivity increase up a group in halogens vs increasing down a group in alkaline/alkaline earth

A

Less outer shells thus higher attraction to nucleas and thus reacts/attracts easier than other

Alkaline, loses electrons so thus more shells means less charge to nucleas and can lsoe easier, reacting with more

75
Q

What elemetns are liquid at room temp

A

Bromine and Mercury

76
Q

Ductile vs Malleable

A

Ductile –> rolled into wire - under tensile stresses
Malleable –> deform or change shape of metal, into sheets

77
Q

Explain metallic bonding

A
  • Ductile and malleable
  • Between metals (can be different e.x. alloys)
78
Q

What is filtering

A

Physcial property –> particle size
particles smaller than filter holes passes through, called the filtrate, while other stuff are left behind

79
Q

What is decanting

A

Physcial property –> density/lack of suluability
pour off a layer of a mixture, leaving other layers behind ex. sandy water/wine

80
Q

Distillation

A

Physcial property –> boiling point
Mixture heated up to the evaporated subastances boiling point, vapour is captured and condensed
seperate missible liquids

81
Q

What is a covalent network solid

A

giant network of covalentley bonded atoms e.x. diamond/graphite

82
Q

What is a seperating funnel

A

seperate immisible liquids by density/layers

83
Q

What is evaporation

A

seperate solute from solvent (salt and water)

84
Q

How is electronegativity related to oxide types?

A

Less electronegative the more likely to be basic (metals) vs covalent who are more electronegative form acidic oxides

Chemistry Unit 1 (2 decks)

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