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Chemistry > Module 1 > Flashcards

Module 1 Flashcards

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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

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

A

Flame Test can be used to indicate the emission spectra

21
Q

Define band of stability

A

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

22
Q

Identify types of radiation

A

Types of Radiation:
- Alpha radiation
- Beta radiation
- Gamma ray

23
Q

Outline features of alpha radiation

A

Alpha Ray:
- Positively charged
- Equivalent to Helium atom
- Heavy; low penetrating power

24
Q

Outline features of beta radiation

A

Beta Ray:
- Negatively charged
- Equivalent to an electron
- Light; medium penetrating power

25
Q

Outline features of gamma rays

A

Gamma Ray:
- Carries no charge
- Negligible mass; high penetrating power

26
Q

Define polarity

A

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
Q

Link polarity and electronegativity

A

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
Q

Define lone pairs

A

Lone Pairs are pairs of electrons that are not bonded to other atoms

29
Q

Define Valence Shell Electron-Pair Repulsion Theory (VSEPR)

A

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
Q

Define allotropy

A

Allotropy are the different forms of a singular element through different structural arrangement

31
Q

Define ionic bonding

A

Ionic Bonding is the exchange of valence electrons between metals and non-metals to achieve a stable electron configuration - forms a lattice structure

32
Q

Identify physical properties of ionic bonding

A

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
Q

Define covalent bonding

A

Covalent Bonding is the sharing of valence electrons between non-metals to achieve a stable electron configuration

34
Q

Identify physical properties of covalent bonding

A

Physical Properties:
- Low boiling and melting points – weak electrostatic forces of attraction
- Inability to conduct electricity – no free moving (delocalised) electrons

35
Q

Define covalent network solid

A

Covalent Network Solid are covalent bonds extends indefinitely throughout the whole crystal in a lattice structure

36
Q

Identify physical properties of covalent network solid

A

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
Q

Define metallic bonding

A

Metallic Bonding has positively charged metal particles surrounded by a sea of delocalised electrons

38
Q

Identify physical properties of metallic bonding

A

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
Q

Identify the types of intermolecular forces in ascending strength

A

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
Q

Electron Shells →…

A

Electron Shells → Subshells → Orbitals

41
Q

Identify the short-hand form of electron configuration

A

Electron Configuration → Noble Gas Configuration

42
Q

Relate the colour from a Flame Test and energy

A

The energy increases from colours - ROY-G-BIV to White

43
Q

Explain why larger molecules have higher boiling points

A

Larger molecules have higher boiling points as they have more nuclei and electrons - dispersion forces, increasing the intermolecular forces

44
Q

State Gay-Lussac’s Law

A

The pressure and temperature of a gas is proportional

45
Q

State Boyle’s Law

A

The pressure and volume of a gas is inversely proportional

46
Q

State Charles’ Law

A

The temperature and volume of a gas is proportional

47
Q

State Avogardo’s Law

A

The number of particles and volume of a gas is proportional

48
Q

Law concerning the proportionality of pressure and temperature of a gas

A

Gay-Lussac’s Law

49
Q

Law concerning the inversely proportionality of pressure and volume of a gas

A

Boyle’s Law

50
Q

Law concerning the proportionality of temperature and volume of a gas

A

Charles’ law

51
Q

Law concerning the proportionality of the number of particles and the volume of a gas

A

Avogardo’s Law

Chemistry (7 decks)

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