Module 1 Flashcards
Define solution
Solution is a homogeneous mixture composed of at least 2 substances
Components of a solution
Components of a Solution:
- Solvent
- Solute
Define solvent
Solvent is the medium that dissolves the solute, forming a solution
Define solute
Solute is the substance dissolved in a solution
Define aqueous solution
Aqueous Solution is a solution with water as the solvent
Identify types of mixtures
Types of Mixtures:
- Suspension
- Colloid
- Solution
Identify the difference between suspension and colloid
Difference between Suspension and Colloid:
- Suspension has larger particles than a colloid
- Suspension is opaque; Colloid is translucent
- Suspension is heterogeneous; Colloid is homogeneous
Define fluid
Fluids are substances with no defined shape; gases and liquids
Define miscibility
Miscibility is the property of liquids to form a homogeneous mixture regardless of concentration
Calculate percentage composition of an element
Mass of Element / Mass of Compound
Identify what occurs if immiscible liquids are mixed
The immiscible liquids form distinct layers, depending on density
Define alloy
Alloy is a mixture of chemical elements of which at least one is a metal
True or False. The suffixes of oxidised ions are “-ite” and “-ate”
Suffix of Oxidised ions: “-ite” and “-ate”; where “-ite” refers to the lower oxidation state
Define anion
Anions are negatively charged ions; usually non-metals
Define mass number
Mass Number (Nucleon Number) is the number of protons and neutrons in an atom
Define cation
Cations are positively charged ions; metals
Define atomic number
Atomic Number is the number of neutrons in an atom
Define octet number
The Octet Rule is a rule that states atoms tend to have 8 electrons in their valence shell
True or False. Orbitals hold a singular electron
False, orbitals can hold 2 electrons – ‘up’ and ‘down’ electron, represented by arrows with the ‘up’ electron filled first
Define the Aufbau Principle
The Aufbau Principle states that electrons occupy the lowest energy orbital
Define 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
Define 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
Define flame test
Flame Test can be used to indicate the emission spectra
Define band of stability
Band of Stability is a region where the nuclei of an atom is stable
Identify types of radiation
Types of Radiation:
- Alpha radiation
- Beta radiation
- Gamma ray
Outline features of alpha radiation
Alpha Ray:
- Positively charged
- Equivalent to Helium atom
- Heavy; low penetrating power
Outline features of beta radiation
Beta Ray:
- Negatively charged
- Equivalent to an electron
- Light; medium penetrating power
Outline features of gamma rays
Gamma Ray:
- Carries no charge
- Negligible mass; high penetrating power
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
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
Define lone pairs
Lone Pairs are pairs of electrons that are not bonded to other atoms
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
Define allotropy
Allotropy are the different forms of a singular element through different structural arrangement
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
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
Define covalent bonding
Covalent Bonding is the sharing of valence electrons between non-metals to achieve a stable electron configuration
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
Define covalent network solid
Covalent Network Solid are covalent bonds extends indefinitely throughout the whole crystal in a lattice structure
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
Define metallic bonding
Metallic Bonding has positively charged metal particles surrounded by a sea of delocalised electrons
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
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
Electron Shells →…
Electron Shells → Subshells → Orbitals
Identify the short-hand form of electron configuration
Electron Configuration → Noble Gas Configuration
Relate the colour from a Flame Test and energy
The energy increases from colours - ROY-G-BIV to White
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
State Gay-Lussac’s Law
The pressure and temperature of a gas is proportional
State Boyle’s Law
The pressure and volume of a gas is inversely proportional
State Charles’ Law
The temperature and volume of a gas is proportional
State Avogardo’s Law
The number of particles and volume of a gas is proportional
Law concerning the proportionality of pressure and temperature of a gas
Gay-Lussac’s Law
Law concerning the inversely proportionality of pressure and volume of a gas
Boyle’s Law
Law concerning the proportionality of temperature and volume of a gas
Charles’ law
Law concerning the proportionality of the number of particles and the volume of a gas
Avogardo’s Law
