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CHEM Y11 > 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
What happans to amphoteric metal oxides
React with both acids and bases to create salts and water
26
How does Sulfer and O2 react in water and where does it come from
Sulfer and Dioxide --> Sulphur Dioxide + Water --> acidic rain sulfer is gained from coal burning
27
How do oxides change from left to right a period and down a group
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)
28
What are three acidic oxides to memorise
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)
29
What happans when Nitrogen Oxide reacts with water and where does it come from
Cars produce nitrogen --> acid rain since caues HNO2 or HNO3 and falls
30
What is H2SO4 or H2SO3
H2SO4 = Sulfuric acid H2SO3 = sulfourius acid
31
What are all the properties of ionic bonds - electricity - structure - force - physical property - Between...
- 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
32
What are all the properties of covalent bonds - electricity - structure - force - physical property - Between...
- 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
33
Acids and bases with electricity?
Strong acids + bases are good conductors and thus good electrolytes
34
Define valency
The power to combine
35
How strong are ionic vs covalent bonds
Ionic bonds are stronger than covalent since harder to break covalent
36
What is the molecular and electronic geomtery + angle of Methane
CH4 - tetrahedral in molecular - tetrahedral in electron geometry 109 degrees
37
What is methane
CH4
38
What is ammonia
NH3
39
What is ammonium
NH4
40
What is the molecular and electronic geomtery + angle of Water
H2O - Bent molecular - tetrahedral electron 104.5 degrees
41
What is the molecular and electronic geomtery + angle of Ammonia
NH3 - Pyramidal molecular - tetrahedral electronic 107 degrees
42
What is it called when a liquid dissolves into a liquid
Miscible
43
What is it called when a solid dissolves into a liquid
Soluble
44
The 3 chemical compounds that are so strong they cant dissolve in water
CaCO3 AgCl BaSO4 Insoluble in water since the bonds are so strong there is not enough energy in the water
45
What are physical properties
observed without a chemical change/changing identity of a substance (melting points, density, malleability, boiling point)
46
What are chemical properties and example
(flammability, corrosion, oxidation, PH, reactivity) - how a substance changes into a different cubstance
47
Patterns of Halogens
Reactivity decreases down, MP,/BP increase down, Density increase down
48
Patterns of alkali metals
Reactivity increases down, MP,BP decrease down, Density increase down, soft, shiny and silver colour
49
What is the pop test
Hydrogen gas test by adding flint to h2 and u get a pop
50
List all diatomic gases, how many are there?
7 --> H, N, O, F, Cl, Br, I Have no fear of ice cold bear
51
What is direct synthesis combination?
2/more substancces react together to form 1 product (A + B --> AB)
52
What is a single replacement reaction?
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
What is combustion?
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
What is a suspension
Heterogeneous mixture of a fluid that contains solid particles sufficiently large for sedimentation
55
What is an alloy
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
What is a solvent in relation to solute
The substance in which a solute dissolves to produce a homogeneous mixture
57
What is a solute
Something that gets dissolved in a solvent like salt or sugar
58
What is a
Something composed of two or more separate elements; a mixture
59
What is a molecule
Two or more atoms held together by bonds
60
Describe the properties of sodium chloride
- 3D dimensional arrangement of +ve & -ve ions (neg Cl and pos Na)
61
Whats the relationship between polarity and electronegativity
The bigger the electronegativity difference the higher polarity
62
What is isoelectronic
Having the same numbers of electrons or the same electronic structure E.x. N3- and Ne and Na+ all have same electorn count
63
What is isoelectronic
Having the same numbers of electrons or the same electronic structure E.x. N3- and Ne and Na+ all have same electorn count
64
What is an allotrope
Each of two or more different physical forms in which an element can exist. Graphite, charcoal, and diamond are all allotropes of carbon.
65
Why is the second ionization energy always higher than the first
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
What is decomposoiton reaction?
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
What is a double replacement reaction?
(AB + CD --> AC + BD) The positive and negative ions in two compounds switch places BaCl2 + NaSO4 --> BaSO4 + NaCl
68
What is a redox/oxidation-reduction reaction?
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
What indicates a chemical reaction
Release of energy as heat Release of energy as light Formation of gas Change in colour Chnage in odour
70
What is a neautralization reaction?
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
What is a neautralization reaction?
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
What is the reactiivyt of elements in periodic table
Metals --> more to left and down = highest Non metals --> more to the right and top = highest (disregarding noble gases and metataloids)
72
What are all reactions
Synthesis Decomposition Double Replacement Single replacement Redox Neutralization Combustion
73
Differnet Ph levels and their meanings
7 = neautral 8 to 14 = base 6 to 0 = acid
74
, Why does reactivity increase up a group in halogens vs increasing down a group in alkaline/alkaline earth
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
What elemetns are liquid at room temp
Bromine and Mercury
76
Ductile vs Malleable
Ductile --> rolled into wire - under tensile stresses Malleable --> deform or change shape of metal, into sheets
77
Explain metallic bonding
- Ductile and malleable - Between metals (can be different e.x. alloys)
78
What is filtering
Physcial property --> particle size particles smaller than filter holes passes through, called the filtrate, while other stuff are left behind
79
What is decanting
Physcial property --> density/lack of suluability pour off a layer of a mixture, leaving other layers behind ex. sandy water/wine
80
Distillation
Physcial property --> boiling point Mixture heated up to the evaporated subastances boiling point, vapour is captured and condensed seperate missible liquids
81
What is a covalent network solid
giant network of covalentley bonded atoms e.x. diamond/graphite
82
What is a seperating funnel
seperate immisible liquids by density/layers
83
What is evaporation
seperate solute from solvent (salt and water)
84
How is electronegativity related to oxide types?
Less electronegative the more likely to be basic (metals) vs covalent who are more electronegative form acidic oxides

CHEM Y11 (2 decks)

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