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Chemistry > Module 1 > Flashcards

Module 1 Flashcards

(54 cards)

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1
Q

Define solution

A

Solution is a homogeneous mixture composed of at least 2 substances

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2
Q

Components of a solution

A

Components of a Solution:
- Solvent
- Solute

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3
Q

Define solvent

A

Solvent is the medium that dissolves the solute, forming a solution

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4
Q

Define solute

A

Solute is the substance dissolved in a solution

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5
Q

Define aqueous solution

A

Aqueous Solution is a solution with water as the solvent

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6
Q

Identify types of mixtures

A

Types of Mixtures:
- Suspension
- Colloid
- Solution

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7
Q

Identify the difference between suspension and colloid

A

Difference between Suspension and Colloid:
- Suspension has larger particles than a colloid
- Suspension is opaque; Colloid is translucent
- Suspension is heterogeneous; Colloid is homogeneous

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7
Q

Define fluid

A

Fluids are substances with no defined shape; gases and liquids

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8
Q

Define miscibility

A

Miscibility is the property of liquids to form a homogeneous mixture regardless of concentration

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9
Q

Calculate percentage composition of an element

A

Mass of Element / Mass of Compound

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9
Q

Identify what occurs if immiscible liquids are mixed

A

The immiscible liquids form distinct layers, depending on density

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10
Q

Define alloy

A

Alloy is a mixture of chemical elements of which at least one is a metal

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11
Q

True or False. The suffixes of oxidised ions are “-ite” and “-ate”

A

Suffix of Oxidised ions: “-ite” and “-ate”; where “-ite” refers to the lower oxidation state

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12
Q

Define anion

A

Anions are negatively charged ions; usually non-metals

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13
Q

Define mass number

A

Mass Number (Nucleon Number) is the number of protons and neutrons in an atom

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13
Q

Define cation

A

Cations are positively charged ions; metals

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14
Q

Define atomic number

A

Atomic Number is the number of neutrons in an atom

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15
Q

Define octet number

A

The Octet Rule is a rule that states atoms tend to have 8 electrons in their valence shell

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16
Q

True or False. Orbitals hold a singular electron

A

False, orbitals can hold 2 electrons – ‘up’ and ‘down’ electron, represented by arrows with the ‘up’ electron filled first

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17
Q

Define the Aufbau Principle

A

The Aufbau Principle states that electrons occupy the lowest energy orbital

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18
Q

Define Hund’s Rule

A

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

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19
Q

Define Pauli Exclusion Principle

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A

Pauli Exclusion Principle states that a maximum of two electrons may occupy a single orbital but only if the electrons have opposite spins

20
Q

Define flame test

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A

Flame Test can be used to indicate the emission spectra

21
Q

Define band of stability

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A

Band of Stability is a region where the nuclei of an atom is stable

22
Identify types of radiation
Types of Radiation: - Alpha radiation - Beta radiation - Gamma ray
23
Outline features of alpha radiation
Alpha Ray: - Positively charged - Equivalent to Helium atom - Heavy; low penetrating power
24
Outline features of beta radiation
Beta Ray: - Negatively charged - Equivalent to an electron - Light; medium penetrating power
25
Outline features of gamma rays
Gamma Ray: - Carries no charge - Negligible mass; high penetrating power
26
Define polarity
Polarity is when an atom has poles and hence has slightly positive and negative charges on opposing ends; indicates the equilibrium of the sharing of electrons
27
Link polarity and electronegativity
Polarity and Electronegativity: - A low difference in electronegativity is a nonpolar covalent bond - A medium difference in electronegativity is a polar covalent bond - A high difference in electronegativity is an ionic bond - Diatomic molecules are nonpolar
28
Define lone pairs
Lone Pairs are pairs of electrons that are not bonded to other atoms
29
Define Valence Shell Electron-Pair Repulsion Theory (VSEPR)
Valence Shell Electron-Pair Repulsion Theory (VSEPR) 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
30
Define allotropy
Allotropy are the different forms of a singular element through different structural arrangement
31
Define ionic bonding
Ionic Bonding is the exchange of valence electrons between metals and non-metals to achieve a stable electron configuration - forms a lattice structure
32
Identify physical properties of ionic bonding
Physical Properties: - High boiling and melting points – strong electrostatic forces of attraction - Hard but brittle – strong electrostatic forces of attraction - Conducts electricity in the molten state – free moving (delocalised) charged particles
33
Define covalent bonding
Covalent Bonding is the sharing of valence electrons between non-metals to achieve a stable electron configuration
34
Identify physical properties of covalent bonding
Physical Properties: - Low boiling and melting points – weak electrostatic forces of attraction - Inability to conduct electricity – no free moving (delocalised) electrons
35
Define covalent network solid
Covalent Network Solid are covalent bonds extends indefinitely throughout the whole crystal in a lattice structure
36
Identify physical properties of covalent network solid
Physical Properties: - High boiling and melting points – strong lattice structure - Inability to conduct electricity – no free moving (delocalised) electrons - Hard and brittle – strong lattice structure
37
Define metallic bonding
Metallic Bonding has positively charged metal particles surrounded by a sea of delocalised electrons
38
Identify physical properties of metallic bonding
Physical Properties: - High boiling and melting points –strong electrostatic forces of attraction - Strong – strong electrostatic forces of attraction - Good conductors of heat and electricity – Free moving (delocalised) charged particles - Malleable and Ductile – Free moving charged particles makes the structure more fluid
39
Identify the types of intermolecular forces in ascending strength
Types of Intermolecular Forces: - Dispersion – an intermolecular force between all molecules - Dipole-dipole – an intermolecular force between polar molecules - Hydrogen bond – an intermolecular force that involves a hydrogen atom bonded to an oxygen, nitrogen, or fluorine atom
40
Electron Shells →...
Electron Shells → Subshells → Orbitals
41
Identify the short-hand form of electron configuration
Electron Configuration → Noble Gas Configuration
42
Relate the colour from a Flame Test and energy
The energy increases from colours - ROY-G-BIV to White
43
Explain why larger molecules have higher boiling points
Larger molecules have higher boiling points as they have more nuclei and electrons - dispersion forces, increasing the intermolecular forces
44
State Gay-Lussac's Law
The pressure and temperature of a gas is proportional
45
State Boyle's Law
The pressure and volume of a gas is inversely proportional
46
State Charles' Law
The temperature and volume of a gas is proportional
47
State Avogardo's Law
The number of particles and volume of a gas is proportional
48
Law concerning the proportionality of pressure and temperature of a gas
Gay-Lussac's Law
49
Law concerning the inversely proportionality of pressure and volume of a gas
Boyle's Law
50
Law concerning the proportionality of temperature and volume of a gas
Charles' law
51
Law concerning the proportionality of the number of particles and the volume of a gas
Avogardo's Law

Chemistry (7 decks)

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