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chemistry yr 11 > mod 1 > Flashcards

mod 1 Flashcards

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1
Q

Definition: Homogenous

A

is a mixture that is consistant throughout

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2
Q

Defintion: Mixture

A

an impure substance consisting of two or more elements or compounds that aren’t chemically bonded (impure homogenous and heterogenous substances)

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2
Q

Definition: Heterogenous

A

is a mixture with inconsistencies throughout

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3
Q

Definition: Solution

A

is a homogenous mixture
minor substance = solute
major substance = solvent

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4
Q

Definition: Colloid

A

a homogenous mixture with fine particles of an insoluble substance dispersed

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5
Q

Definition: suspension

A

is a heterogeneous mixture where large particles don’t dissolve in the solvent and sediment overtime

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6
Q

Definition: Gravimetric analysis/percentage composition

A

works out the composition of a mixture (write to the lowest sig figs in the question)

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7
Q

How are ionic bonds formed?

A

they are formed by the electrostatic attraction between cations (+) and anions (-) (metal and non metal)

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8
Q

How are covalent bonds formed?

A

they are formed when 2 or more elements (non-metals) share a pair of electrons

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9
Q

Memorise the polyatomic ions/radicals

A

nitrate/nitrite
hydroxide
hydrogen carbonate
carbonate
sulfate/sulfite
phosphate
ammonium/ammonia

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10
Q

Name some physical properties (properties observed without changing chemical properties or matter)

A

melting point
boiling point
lustre
malleability
ductility
electrical/thermal conductivity

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11
Q

Name the liquid and gas elements at room temperature (25C)

A

liquids: bromine, mercury
gases: helium, neon, argon, krypton, xenon, raden (noble gases), hydrogen, nitrogen, oxygen, fluorine, chlorine

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12
Q

Name some chemical properties (can be observed when a substance undergoes a chemical reaction to form a new compound)

A

reactivity

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13
Q

What is the flame test?

A

Flame tests are used to identify a certain cation through their distinctive colours as heat transitions the excited atoms to a higher energy level.
lithium = red
sodium = yellow-orange
potassium = purple
calcium = brick-red
barium = apple green
strontium = red
copper = blue green

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14
Q

Definition: Isotopes

A

the same element with a different number of neutrons but same number of protons. they usually give off radioactive decay

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15
Q

Definition: relative atomic mass

A

is the ratio of the weighted average of all natural isotopes of an element to one unit
= (mass of isotope 1 x % of frequency) + (mass of isotope 2 x % of frequency)

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16
Q

What is the empirical formula?

A

simplest ratio between different atoms

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17
Q

How to the lewis diagram for an draw ionic compounds?

A

using brackets + charges + showing full valency

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18
Q

How to draw the lewis diagram for covalent compounds?

A

showing bonds between as pairs electrons + showing valence electrons (both using dots or crosses)

19
Q
  1. 2BG + 0LP - linear
  2. 3BG + 0LP - trigonal planar
  3. 2BG + 1LP - trigonal planar
  4. 4BG + 0LP - tetrahedral
  5. 3BG + 1LP - tetrahedral
  6. 2BG + 2LP - tetrahedral
  7. 5BG + 0LP - trigonal bipyramidal
  8. 6BP + 0LP - octahedral
A
  1. linear
  2. trigonal planar
  3. bent
  4. tetrahedral
  5. trigonal pyramidal
  6. bent
  7. trigonal bipyramidal
  8. octahedral
20
Q

What are ionic networks?

A

a 3D lattice consist of cations and anions that are bonded by electrostatic attraction
- hard, brittle, high melting/boiling
- can only conduct electricity in aqueous form

21
Q

What are covalent networks?

A

are extensive networks/chains of atoms bonded by strong covalent bonds
- very hard, brittle, high melting/boiling
- not electrical conductors

22
Q

What are metallic structures? (metals)

A

are 3D lattices of metal cations in a sea of delocalised valence electrons
- hard (softer than other networks), flexible, high melting/boiling, lustrous
- conduct electrivity

23
Q

What are covalent molecular structures?

A

are composed of discrete covalent molecules with no chemical bonds between them, but held by weaker intermolecular forces
- soft, flexible OR brittle, low boiling/melting
- do not conduct electricity

24
Q

What is the absorption spectrum?

A

is produced when white light is passed through an element which absorbs specific wavelengths of light and leaves dark lines on a coloured spectrum

25
Q

What is the emission spectrum?

A

is produced when an element is heated and electrons excite and de-excite producing coloured lines on a dark spectrum

26
Q

What is rutherford’s model of the atom?

A
27
Q

What is bohr’s model of the atom?

A
28
Q

What is schrodinger’s model of the atom?

A
29
Q

What is Effective Nuclear Charge? (ENC)

A

Z(eff) = no. of protons - shielding electrons (no. of electrons blocking the chosen electron, therefore total electrons - it’s current shell’s no. of electrons)

30
Q

What is the ENC’s trend?

A

Across a period: increases
Down a group: decreases

31
Q

What is electronegativity?
What is 1st ionisation energy?

A

the ability for the nucleus to attract a pair of electrons
the energy needed to remove a valence electron

32
Q

What is the electronegativity and 1st ionisation energy trend?

A

across a period: increases
down a group: decreases

33
Q

What are the reactivity trends?

A

group 1-2 metals: more reactive down the group
group 7: mildy reactive and increase down the group

34
Q

Ionic bonds are created between ____

A

elements with a large difference in electronegativity (>1.8)(metals and non metals)

35
Q

Polar (electrons are slighty tilted towards the more electronegative element - dipole moment) covalent bonds are created between ____

A

elements with a moderate difference in electronegativity (0.4-1.8)
e.g OH, HF, NH, SO, CCl

36
Q

Non-polar covalent bonds are created between ___

A

elements with a small/no difference in electronegativity (<0.4)

37
Q

What are allotropes?

A

are different structures of the same element in the same state although with different physical properties (e.g carbon, oxygen, boron, iron)

38
Q

What are the 3 carbon allotropes?

A
  • graphite (layers of covalent networks bonded ontop of each other using intermolecular forces)
  • diamond (complex covalent network, each carbon atom is bonded to 4 others with no lone pairs)
  • buckminsterfullerene (covalent molecular structure, a large ball of 60 carbon atoms covalent bonded together and then bonded to other balls using intermolecular forces)
39
Q

Polarity of molecules depends on ___

A
  1. polarity of bonds (if there are no polar bonds the whole molecule is non-polar)
  2. molecular geometry (make sure that the charges don’t cancel each other out)
40
Q

What are the 3 types of intermolecular forces? weakest to strongest.

A
  1. dispersion forces (electrons randomly moving around to cause a temporary dipole moment)(exists between ANY molecules)
  2. dipole-dipole forces (have a net dipole slightly + or - and force grows stronger with larger difference in electronegativity)(exist between POLAR molecules)
  3. hydrogen bonding (directly to the highly electronegative atoms and because hydrogen is so small, it can squeeze in)(between F, O, N and H)
41
Q

Definition: Kinetic particle theory

A

a theory that states that all matter is composed of particles in motion and that the rate of motion varies directly with the temperature.

42
Q

Oxidation/reduction reaction (metals, think abt the transfer of electrons)

A

half reactions in a reaction
OXIDATION: increases the charge of the element in the product from the reactant
REDUCTION: decreases the charge of the element in the product from the reactant
e.g Mg+O2=MgO (magnesium oxidised from 0 to +2)(oxygen reduced from 0 to -2)

43
Q

metal + water = ____

A

metal hydroxide + hydrogen gas
(break into equation into ions and decide which element is oxidised and which is reduced)

44
Q

acid + metal carbonate = ___

A

salt + water + CO2

45
Q

(neutralisation) acid + base = ___

A

salt + water

46
Q

NAG SAG (always soluble)

A

nitrates
acetates
group 1

sulfates
ammonium
group 7

EXCEPTION: SILVER, LEAD AND MERCURY (always insoluble)

chemistry yr 11 (4 decks)

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