Year 11 Chemistry Comprehensive Flashcards

0.0(0)
studied byStudied by 2 people
learnLearn
examPractice Test
spaced repetitionSpaced Repetition
heart puzzleMatch
flashcardsFlashcards
Card Sorting

1/84

flashcard set

Earn XP

Description and Tags

Vocabulary flashcards for Year 11 Chemistry.

Study Analytics
Name
Mastery
Learn
Test
Matching
Spaced

No study sessions yet.

85 Terms

1
New cards

Who was J.J. Thomson and what did he discover?

Joseph John Thomson was a British physicist who won the Nobel Prize in 1906. He discovered the electron and proposed the plum pudding model of the atom.

2
New cards

Thomson's cathode-ray tube experiment led him to conclude that _ were present in all types of matter.

electrons

3
New cards

What did Rutherford contribute to atomic theory?

Rutherford discovered that atoms have a small, dense, positively charged center (nucleus) with electrons moving around the outside.

4
New cards

What is the plum pudding model?

Thomson's model of the atom where electrons (like plums) are embedded in a positively charged sphere (like pudding).

5
New cards

According to Schrödinger, electrons exist in _.

shells

6
New cards

What subatomic particle did Chadwick discover?

The neutron

7
New cards

Fill in the missing information: Proton: Location = ?, Charge = +1, Mass = 1 Neutron: Location = Nucleus, Charge = ?, Mass = 1 Electron: Location = ?, Charge = -1, Mass = ?

Proton: Location = Nucleus Neutron: Charge = 0 Electron: Location = Rapidly moving around the nucleus, Mass = 1/1836

8
New cards

Calculate the number of neutrons in Sodium (Na) if atomic number = 11 and mass number = 23.

Neutrons = Mass number - Atomic number = 23 - 11 = 12 neutrons

9
New cards

The formula for calculating neutrons is: Neutrons = -

Mass number - Atomic number (or protons)

10
New cards

What determines the identity of an atom?

The number of protons (atomic number) determines the identity of an atom.

11
New cards

What is analytical chemistry?

Analytical chemistry involves the use of techniques to obtain information about chemical substances.

12
New cards

_______ analysis is the identification of elements or compounds present in a sample, while _______ analysis determines the amounts

Qualitative; Quantitative

13
New cards

Name 3 techniques used in quantitative analysis.

Any 3 of: Atomic Absorption Spectroscopy, UV-visible spectroscopy, infrared spectroscopy, chromatography, nuclear magnetic resonance, mass spectroscopy

14
New cards

What are flame tests an example of?

Emission spectroscopy

15
New cards

Normally atoms are in the " _ state" where electrons are in the lowest possible energy level.

ground

16
New cards

What happens when atoms absorb energy?

Electrons jump to higher energy levels, creating an "excited state" which is unstable. Electrons quickly return to ground state, releasing energy as light.

17
New cards

What is an absorption spectrum?

A series of dark lines superimposed on a continuous spectrum, showing wavelengths of light that have been absorbed.

18
New cards

What is an emission spectrum?

A series of bright lines against a black background, showing wavelengths of light that have been emitted.

19
New cards

Match the metal ion with its flame color: Sr²⁺, K⁺, Na⁺, Ba²⁺, Cu²⁺ Colors: Red, Orange, Yellow, Green, Pinkish orange

Sr²⁺ = Red, K⁺ = Pinkish orange, Na⁺ = Orange, Ba²⁺ = Yellow, Cu²⁺ = Green

20
New cards

What is AAS used for in industry?

Monitoring the purity of substances (air, water, food), measuring metal ion concentrations at trace levels (ppm or ppb).

21
New cards

In AAS, the higher the concentration of metal in the sample, the _ the absorption.

greater

22
New cards

List the 6 steps for using AAS.

Choose correct lamp for the metal, 2. Make standards with known concentrations, 3. Test standards and record absorbance, 4. Draw calibration curve (concentration vs absorbance), 5. Test unknowns and record absorbance, 6. Use calibration curve to determine concentration

23
New cards

What does the nebulizer do in AAS?

Sucks up samples at controlled rate, creates fine aerosol spray, and mixes aerosol with fuel and oxidant for introduction into flame.

24
New cards

What is the function of the monochromator in AAS?

Separates thousands of lines to select the specific wavelength absorbed by the sample and exclude other wavelengths.

25
New cards

What is mass spectrometry used for?

An instrument to separate particles with different masses and determine relative proportions of particles in a mixture.

26
New cards

Name 4 uses of mass spectrometry.

Find composition of mixtures, 2. Determine molecular structures, 3. Find isotopic composition and atomic mass, 4. Detect impurities/viruses

27
New cards

What are the 4 main steps in mass spectrometry?

Ionization (knock off electrons to create positive ions), 2. Acceleration (same kinetic energy), 3. Deflection (by magnetic field based on mass), 4. Detection (electrical detection)

28
New cards

In mass spectrometry, lighter ions are deflected _ than heavier ions.

more

29
New cards

Calculate the relative atomic mass of Bromine using MS data: ⁷⁹Br (50% abundance) and ⁸¹Br (50% abundance).

Mr(Br) = ((79×50) + (81×50))/100 = 80

30
New cards

What is atomic radius?

The size of an atom, including the nucleus, electrons, and all empty space in the atom.

31
New cards

Atomic radius depends on 3 things: number of ____, position of electrons in_____ , and ____on nucleus.

electrons; shells; charge

32
New cards

How does atomic radius change down a group and across a period?

Down a group: increases (more electron shells); Across a period: decreases (stronger nuclear attraction)

33
New cards

What is electronegativity?

An atom's ability/attraction to electrons.

34
New cards

____is the most electronegative atom, and ______ is the least electronegative.

Fluorine; Francium

35
New cards

How does electronegativity change down a group and across a period?

Down a group: decreases (outer electrons further from nucleus); Across a period: increases (stronger nuclear attraction)

36
New cards

What is ionization energy?

The amount of energy needed to remove an electron from an atom.

37
New cards

Low ionization energy means it's____ to remove an electron, while high ionization energy means it's _____to remove an electron.

easy; hard

38
New cards

How does ionization energy change down a group and across a period?

Down a group: decreases (weaker attraction); Across a period: increases (stronger nuclear attraction)

39
New cards

Why do successive ionization energies increase for the same atom?

Each electron is being removed from an increasingly positive ion, and there's a large jump when removing from a shell closer to the nucleus.

40
New cards

What is electron affinity?

The energy change when an atom gains electrons; the ability of an atom in gaseous state to accept an electron.

41
New cards

What is metallic bonding?

The electrostatic attraction between positive metal cations and delocalised electrons in a 3D lattice.

42
New cards

Metallic bonding occurs between _ atoms only.

metal

43
New cards

Name 5 properties of metallic bonding and explain one.

Conduct heat/electricity, 2. Hardness, 3. Malleability/ductility, 4. High melting/boiling points, 5. Lustre.

44
New cards

What is ionic bonding?

Electrostatic attraction between oppositely charged ions arranged in a 3D lattice, formed between metal and non-metal.

45
New cards

In ionic bonding, metals electrons to become , while non-metals electrons to become .

lose; cations; gain; anions

46
New cards

Why are ionic compounds hard but brittle?

Hard due to strong attraction between ions; brittle because when layers slide, like charges repel causing shattering.

47
New cards

Why don't ionic solids conduct electricity, but ionic liquids do?

Solids have fixed ion positions (can't move), but in liquids/solutions ions are free to move and carry charge.

48
New cards

What is covalent bonding?

Electrostatic attraction between positive nuclei and shared pair(s) of electrons, formed between non-metals.

49
New cards

A single covalent bond involves shared electrons, a double bond involves , and a triple bond involves _.

2 (1 pair); 4 (2 pairs); 6 (3 pairs)

50
New cards

Compare melting points: covalent molecular vs covalent network.

Covalent molecular: Low (weak intermolecular forces); Covalent network: Very high (must break strong covalent bonds)

51
New cards

Why is graphite a conductor but diamond isn't?

Graphite has delocalised electrons (4th electron per carbon) free to move between layers; diamond has all electrons in covalent bonds.

52
New cards

What are some examples of network covalent substances?

Diamond, graphite, carbon (as graphite or diamond), carbon dioxide, silicon, boron, silicon carbide, and silicon nitride.

53
New cards

What steps should you follow when justifying bonding properties?

Type of bond, 2. Lattice type, 3. Intermolecular forces, 4. Nuclear attraction, 5. Delocalised electrons, 6. Bond definition, 7. Directional bonds, 8. Property explanation

54
New cards

Justify why silver is malleable.

Silver has metallic bonding with delocalised electrons in a "sea" around cations in 3D lattice. Strong electrostatic attraction forms non-directional bonds. Layers can slide past each other while maintaining the metallic lattice due to non-directional bonding.

55
New cards

Justify why diamond is very hard.

Diamond is a covalent network with each carbon covalently bonded to 4 others in 3D lattice. Strong intramolecular forces (covalent bonds) require lots of energy to disrupt and break apart.

56
New cards

What size range defines nanomaterials?

1nm to 999nm

57
New cards

Name 4 properties of nanoparticles.

High elasticity, high thermal conductivity, low density, chemically more inert

58
New cards

Name 3 uses of nanotechnology.

Drug delivery, sensing, water treatment

59
New cards

Name 3 environmental concerns about nanoparticles.

Can accumulate for long periods, move up food chain, harm ecosystems, alter microbial processes, leach into water/soil

60
New cards

What are hydrocarbons?

Organic compounds containing only carbon and hydrogen atoms.

61
New cards

Carbon has electrons in outer shell and needs to form bonds to be stable.

4; 4

62
New cards

Define empirical, molecular, and structural formulas.

Empirical: smallest whole number ratio; Molecular: actual ratio; Structural: arrangement of atoms (drawn)

63
New cards

What are the two main types of hydrocarbons?

Aromatic (contain benzene rings) and Aliphatic (no benzene rings)

64
New cards

What is benzene and how is it represented?

C₆H₆, most important aromatic hydrocarbon, represented as hexagon with circle inside showing 6 delocalised electrons

65
New cards

What is the general formula for alkanes?

CnH₂n+₂

66
New cards

What makes alkanes "saturated"?

They contain only single bonds between carbon atoms.

67
New cards

Give the prefixes for 1-8 carbons.

1=meth, 2=eth, 3=prop, 4=but, 5=pent, 6=hex, 7=hept, 8=oct

68
New cards

What makes alkenes "unsaturated"?

They contain at least one double bond between carbon atoms.

69
New cards

Name the alkyl groups: CH₃-, CH₂CH₃-, CH₂CH₂CH₃-

Methyl, Ethyl, Propyl

70
New cards

Give the prefixes for: Fluorine, Chlorine, Bromine, Iodine

Fluoro, Chloro, Bromo, Iodo

71
New cards

Name 3 general properties of hydrocarbons.

Low melting/boiling points, colourless, often no odor (simple ones)

72
New cards

What is the formula for cycloalkanes and cycloalkenes?

Cycloalkanes: CnH₂n ; Cycloalkenes: CnH₂n-₂

73
New cards

What are the products of complete vs incomplete combustion?

Complete: CO₂ + H₂O; Incomplete: CO + H₂O

74
New cards

Carbon monoxide is ______ and _______.

colourless; odourless

75
New cards

What is an exothermic reaction?

A reaction that releases heat energy to surroundings, temperature increases, energy released > energy required, ΔH is negative.

76
New cards

What is an endothermic reaction?

A reaction that takes in heat from surroundings, temperature decreases, energy required > energy released, ΔH is positive.

77
New cards

Breaking bonds ____energy, while forming bonds______ energy.

takes/requires; releases

78
New cards

State the law of conservation of energy.

Energy cannot be created or destroyed, only transferred. All energy lost or gained must go or come from somewhere.

79
New cards

How can you tell if a reaction is exothermic or endothermic from an energy diagram?

Exothermic: products lower than reactants (energy released); Endothermic: products higher than reactants (energy absorbed)

80
New cards

In the equation: A + B → C + D + 150kJ, is this exothermic or endothermic?

Exothermic (heat is a product, energy released)

81
New cards

Complete the trend summary: Atomic radius: ↑ down, ↓ across Electronegativity: ↓ down, ↑ Ionization energy: ↓ , ↑ across

across; down

82
New cards

Match bonding type with conductivity: Metallic, Ionic solid, Ionic liquid, Covalent molecular, Covalent network Options: Conductor, Non-conductor

Metallic: Conductor; Ionic solid: Non-conductor; Ionic liquid: Conductor; Covalent molecular: Non-conductor; Covalent network: Non-conductor (except graphite)

83
New cards

Why are Group 1 & 2 metal compounds usually white/colorless while transition metal compounds are colored?

Group 1 & 2 metals form simple ionic compounds, while transition metals have partially filled d-orbitals that can absorb visible light.

84
New cards

Name one technique each for qualitative and quantitative analysis.

Qualitative: Flame tests; Quantitative: Atomic Absorption Spectroscopy (AAS)

85
New cards

What information can mass spectrometry provide about bromine isotopes?

The relative abundance of ⁷⁹Br and ⁸¹Br isotopes, allowing calculation of average atomic mass (≈80 amu).