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Y11: Chem > Module 1 > Flashcards

Module 1 Flashcards

1
Q

Define inquiry question

A

Inquiry Question is a question that focuses on a researchable issue whose answer takes the form of a claim that is supported by evidence, information, and reasoning

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2
Q

Define hypothesis

A

Hypothesis is a proposed explanation for a phenomenon, includes cause and effect language

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3
Q

Define aim

A

Aim is a statement outlining the purpose of the experiment

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4
Q

Define discussion

A

Discussion discusses whether the experiment addressed the hypothesis and aim

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5
Q

Define conclusion

A

Conclusion is a concise summary of ideas and results that have been forementioned and hence it never introduces any new ideas or results

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6
Q

Recall the features of a conclusion

A

Features of a conclusion:
- Briefly restate the purpose of the experiment (i.e. the question it was seeking to answer)
- Identify the main findings (i.e. the answer to the research question)
- Note the main limitations that are relevant to the interpretation of the results
- Summarise what the experiment has contributed to the broader understanding of the problem

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7
Q

Define independent variable

A

Independent Variable is the variable that is changed; on the x-axis

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8
Q

Define dependent variable

A

Dependent Variable is the variable that may be affected by the independent variable and is measured; on the y-axis

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9
Q

Define controlled variable

A

Controlled Variables are the variables that are kept constant

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10
Q

Define qualitative variables

A

Qualitative Variables are the variables that are observed and cannot be measured

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11
Q

Define quantitative variables

A

Quantitative Variables are the variables that are measured

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12
Q

Define validity

A

Validity refers to whether an experiment or investigation is in fact testing the set hypothesis and aims

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13
Q

Define reliability

A

Reliability refers to the idea that an experiment can be repeated many times and the average of the results from all the repeated experiments will be consistent

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14
Q

Define accuracy

A

Accuracy is the ability to obtain the correct measurement. To obtain accurate results, you must minimise systematic errors

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15
Q

Define precision

A

Precision is the ability to consistently obtain the same measurement. To obtain precise results, you must minimise random errors

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16
Q

Define risk assessment

A

Risk Assessment determines the risks of an experiment and the means of damage and controlling it

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17
Q

Recall the features of a risk assessment

A

Features of a risk assessment:
- Risk
- Hazard
- Control

Alternatively,
- Identify
- Assess
- Control

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18
Q

Define uncertainty

A

Uncertainty is the plausible variation of the data represented with ±

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19
Q

Recall the types of errors

A

The types of errors are:
- Systematic Error
- Random Error
- Gross Error

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20
Q

Define systematic error

A

Systematic Error is an error that causes a consistent shift of the data in a singular direction

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21
Q

Define random error

A

Random Error is an error that is unpredictable and caused unknowingly and as the name suggests has no pattern

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22
Q

Define gross error

A

Gross Error is an outlier and usually arises from human incompetence

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23
Q

Define pure substance

A

Pure Substance is a substance that is not contaminated by any other substances

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24
Q

Define impure substance

A

Impure Substance is a substance that is contaminated with traces of other substances

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25
Recall an alternate term for impure substance
Mixture is an alternate term for impure substance
26
Define homogenous
Homogenous means “of uniform composition throughout”
27
Define heterogenous
Heterogeneous means “having non-uniform composition”
28
Define element
Element is a pure substance that cannot be decomposed into simpler substances
29
Define compound
Compound is a pure substance that can be decomposed into simpler substances
30
True or False: Heterogenous substances are always mixtures
True
31
Define kinetic particle theory
Kinetic Particle Theory states that all matter is formed of tiny particles. The particles are constantly randomly moving about. The particles can be arranged regularly or randomly. The particles are held together by weak or strong forces
32
Define subatomic particles
Subatomic Particles are particles that are smaller than an atom; protons, neutrons, and electrons
33
Define solution
Solution is a homogeneous mixture composed of at least 2 substances
34
Recall the components of a solution
Components of a Solution - Solvent - Solute
35
Define solvent
Solvent is the medium that dissolves the solute, forming a solution
36
Define solute
Solute is the substance dissolved in a solution
37
Define aqueous solution
Aqueous Solution is a solution with water as the solvent
38
Recall the types of mixtures
Types of Mixtures - Suspension - Colloid - Solution
39
Define suspension
Suspensions are heterogeneous mixtures with small insoluble particles that are suspended in the solution
40
Define colloid
Colloids are homogeneous mixtures with small insoluble particles that are suspended in the solution
41
Differentiate between colloids and suspensions
The main difference between a suspension and a colloid is when viewed with the naked eye, a suspension is opaque and colloids are translucent or transparent. Hence, in other words, a suspension have larger particles than a colloid Colloids are also homogenous and suspensions are heterogenous and this can be explained through particle size
42
True or False: Pure substances are homogenous
True
43
Define melting
Melting is when a solid changes to a liquid
44
Recall an alternate term for melting
Fusion is an alternate term for melting
45
Define freezing
Freezing is when a liquid changes to a solid
46
Recall an alternate term for freezing
Solidification is an alternate term for freezing
47
Define boiling
Boiling is when a liquid changes to a gas or vapour with the formation of bubbles
48
Define evaporation
Evaporation is when a liquid changes to a gas or vapour without the formation of bubbles
49
Recall an alternate term for evaporation
Vapourisation is an alternate term for evaporation
50
Define condensation
Condensation is when a gas or vapour changes to a liquid
51
Recall an alternate term for condensation
Liquefaction is an alternate term for condensation
52
Define sublimation
Sublimation is when a solid changes to a gas
53
Define fluids
Fluids are substances with no defined shape; gases and liquid
54
Define immiscible
Immiscible is when liquids, if mixed, do not form a homogeneous liquid but instead stay separate in distinct layers, depending on density
55
Define miscible
Miscible is when liquids, if mixed, form a homogeneous liquid
56
Define gravimetric analysis
Gravimetric Analysis determines the quantities of mass of the components
57
Recall the formula to calculate the percentage composition of an element in a compound
Mass of element / Mass of compound *100
58
Recall the features of metals
Features of Metals: - Lustrous - Malleable - Ductile - Dense - High melting and boiling points - High tensile strength - Good conductors of electricity and heat
59
Define alloy
Alloy is a mixture of chemical elements of which at least one is a metal
60
Differentiate between physical and chemical properties
Physical and chemical properties differ in that physical properties are ones that can be measured and observed. On the other hand, chemical properties are related to chemical change
61
Recall physical properties
Physical properties include: - Homogeneous/ Heterogeneous - Colour - Magnetism - Particle Size - Melting and Boiling Points - Density
62
Recall what black lines on a spectra represent
Black lines represent the absorption of a frequency of light in an absorption spectra
63
Recall what coloured lines on a spectra represent
Coloured lines represent the emission of a frequency of light in an emission spectra
64
Recall the schools of thought regarding spectra
Bohr model and Schrödinger's equation
65
Define cation
Cations are positively charged particles
66
Define anion
Anions are negatively charged particles
67
Define mass number
Mass Number is the number of protons and neutrons in an atom
68
Recall an alternate term for mass number
Nucleon Number is an alternate term for mass number
69
Define atomic number
Atomic Number is the number of protons in an atom
70
Define ground state
Ground State is the lowest energy state of an electron
71
Define excited state
Excited State is when an electron absorbs energy and jumps to a higher energy state (electron shell)
72
Recall the octet rule
The Octet Rule is a rule that states atoms tend to have 8 electrons in their valence shell
73
Recall Aufbau Principle
The Aufbau Principle states that electrons occupy the lowest energy orbital
74
Recall Hund's Rule
Hund’s Rule states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals
75
Recall Pauli Exclusion Principle
Pauli Exclusion Principle states that a maximum of two electrons may occupy a single orbital but only if the electrons have opposite spins
76
Define electron configuration
Electron Configuration is a form of displaying the electron structure of an element
77
Define noble gas configuration
Noble Gas Configuration is a niche form of electron configuration, where you state the respective noble gas to make it shorter
78
Recall what each of the following indicates in a mass spectrum: - The number of peaks - The horizontal axis - The vertical axis
Mass Spectrum: - The number of peaks indicates the number of isotopes - The horizontal axis indicates the relative mass of each isotope present in an element according to the isotope’s mass-to-charge ratio (m/z or m/e) - The vertical axis indicates the abundance of each isotope in the sample
79
Define flame test
Flame Test is a simple method that can be used to determine the identity of a metal in a sample
80
Define emission spectrum
Emission Spectrum is a visual representation of the visible light spectrum with coloured lines indicating the release of electromagnetic radiation when the electrons are in the excited state. Each element has a unique spectra
81
Define absorption spectrum
Absorption Spectrum is a visual representation of the visible light spectrum with black lines indicating the absorption of electromagnetic radiation when the electrons jump up in the excited state. Each element has a unique spectra
82
Define Band of Stability
Band of Stability is a region where the nuclei of an atom is stable
83
Recall the types of radiation
Types of Radiation: - Alpha radiation - Beta radiation - Gamma radiation
84
Define nuclear equation
Nuclear Equation is an equation that show radioactive disintegration
85
Define half-life
Half-life is the time required for half the atoms in a given sample to undergo radioactive decay
86
Define polarity
Polarity is when an atom has poles and hence has slightly positive and negative charges on opposing ends
87
Recall the types of polarity
Types of Polarity: - Nonpolar Covalent Bond - Polar Covalent Bond - Ionic Bond
88
True or False: Diatomic molecules are polar
False. Diatomic molecules are always nonpolar
89
Define Lewis Dot Diagram
Lewis Dot Diagram is a means to simply draw the bonding structure of molecules
90
Recall an alternate term for Lewis Dot Diagram
An alternate term for Lewis Dot Diagram is Electron Dot Formula
91
Define lone pairs
Lone Pairs are pairs of electrons that are not bonded to other atoms
92
Recall Valence shell electron-pair repulsion theory
Valence shell electron-pair repulsion theory states the lone pairs in the molecule repel each other and take up positions as far from one another as possible in a 3D space, causing the phenomenon of bent molecules
93
Define allotropes
Allotropes are the different forms of a singular element through different structural arrangement
94
Recall types of intermolecular force
Types of Intermolecular Forces: - Dipole-dipole - Dispersion - Hydrogen bond
95
Define dipole-dipole
Dipole-dipole is an intermolecular force between polar molecules
96
Define dispersion forces
Dispersion forces are an intermolecular forces between all molecules
96
Define dispersion forces
Dispersion forces are an intermolecular forces between all molecules
97
Define hydrogen bonding
Hydrogen bonding is an intermolecular force that involves a hydrogen atom bonded to an oxygen, nitrogen, or fluorine atom
98
Define intramolecular bonds
Intramolecular Bonds are bonds within a molecule
99
Define intermolecular bonds
Intermolecular Bonds are bonds between molecules

Y11: Chem (8 decks)

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