Studied by 9 peopleCompounds have ______________ from their component elements
Different properties
Mixtures contain more than _________________ that are _______ chemically bonded together
One element and/or compound that are not chemically bonded together
Mixtures retain their _____________________ from physically bonded elements/compounds
Individual properties
Mixtures can either be…
Homogeneous or heterogenous
What does homogeneous mean?
The same kind
What does heterogenous mean?
Different in kind
The mole is a fixed number and refers to the __________________ of substance
Amount
Masses of atoms are compared on a scale relative to _____________ and are expressed in Ar (relative atomic mass) and Mr (relative molecular mass)
12^C
The empirical formula of a compound gives the ______________________________ present in a molecule
Simplest ratio of atoms
The molecular formula of a compound gives the ______________________________ present in a molecule
Actual number of atoms
Avogadro’s law enables the mole ratio of reacting gases to be determined from the _______________________ of the gases
Volumes
Describe the nucleus of an atom
Positively charged dense nucleus
The mass spectrometer is used to determine the _______________________ of an element from its isotopic composition
Relative atomic mass
The mass of the electron can be considered _________________
Negligible
Emission spectra are produced when photons are emitted from atoms as _______________________
Excited electrons return to a lower energy level
The line Emission Spectrum of Hydrogen provides evidence for the existence/evidence of ……………….. in ……………… energy levels.
Electrons in discrete energy levels
Which elements have the electron configuration exceptions
Cr and Cu
In an Emission Spectrum, the limit of convergence at higher frequency corresponds to the _____________________________
First ionization energy
Trends in first ionization energy across periods account for the _______________________________ in atoms
Existence of main energy levels and sub-levels
A continuous spectrum in the visible region contains all the ___________ of the spectrum
Colours
A line spectrum (emission/absorption) only shows ___________ frequencies (Quantized)
Certain
The broad trend is that oxides change from ________________________ across a period
Bases from amphoteric to acidic
What is the trend for Atomic radius?
Increases down a group, decreases across a period
What is the trend for Ionic radius?
Increases with increasing negative charge, decreases with increasing positive charge
What is the trend for Ionization energy?
Increases across a period, decreases down a group
What is the trend for Electron Affinity?
Increases across a period, decreases down a group
What is the trend for Electronegatively
Increases across a period, decreases down a group
Diamagnetism is when the atoms of diamagnetic materials have _______ electrons
Paired
Paramagnetism is when the atoms of paramagnetic materials have _______ electrons
Unpaired
The d-sublevel splits into _____________________________ of different energy in a complex ion
Two sets of orbitals
Complexes of d-block elements are coloured, as _________ is absorbed an electrons become ___________ between d-orbitals
Light is absorbed an electrons become excited between d-orbitals
The color absorbed is _____________________ to the color observed
Complementary
Positive ions (cations) form by metals _________ valence electrons
Loosing
Negative ions (anions) form by non-metals _____________ electrons
Gaining
The ionic bond is due to ____________________ attraction between _____________ charged ions
Electrostatic attraction between oppositely charged ions
Under normal conditions, ionic compounds are usually _______ with ____________ structures
solids with lattice structures
What is the name of NH4^+
Ammonium
What is the name of OH^-
Hydroxide
What is the name of NO3^-
Nitrate
What is the name of HCO3^-
Bicarbonate
What is the name of SO4^2-
Sulphate
What is the name of PO4^3-
Phosphate
A covalent bond is formed by the ___________________ attraction between a _________________ of electrons and the _______________________________
Electrostatic attraction between a shared pair of electrons and the positively charged nuclei
Bond polarity results in the difference in _____________________ of the bonded atoms
Electronegativities
The “octet rule” refers to the tendency of atoms to gain a __________________ with a total of ____ electrons
Valence shell with a total of 8 electrons
Some atoms like _____ and ______ might form stable compounds with incomplete octets of electrons
Beryllium and Boron
Resonance structures occur when there is more than _______________for a __________________ in a molecule
one possible position for a double bond
Carbon and Silicon form __________________________ structures
Giant covalent structures
Coordinate Covalent Bonding is a ___________ pair of electrons that originate from a ___________ atom
A shared pair of electrons that originate from a single atom
Electron Geometry of 2 Bonding Pairs
Linear
Electron Geometry of 3 Bonding Pairs
Trigonal Planar
Electron Geometry of 4 Bonding Pairs
Tetrahedral
Molecular Geometry of 2 Bonding Pairs AND 1 Lone Pair
Bent
Molecular Geometry of 3 Bonding Pairs AND 1 Lone Pair
Trigonal Pyramidal
Molecular Geometry of 2 Bonding Pairs AND 2 Lone Pair
Bent
Bond Angle of Tetrahedral Geometry
109.5
Bond Angle of Trigonal Planar Geometry
120
Bond Angle of Linear Geometry
180
For every lone pair present in a molecule, subtract the bond angle by _____
2 or 2.5
A metallic bond is the ___________________ attraction between a lattice of ____________________ and __________________ electrons
Electrostatic attraction between a lattice of positive ions and delocalized electrons
The strength of a metallic bond depends on the ___________ of the ions and the ________ of the metal ion
Charge of the ions and the radius of the metal ion
Alloys usually contain more than one __________ and have ______________ properties
Metal and have enhanced properties
A sigma bond is formed by the ____________ overlap of atomic orbitals
Head on
A pi bond is formed by the ____________ overlap of atomic orbitals
Sideways
Formula for Formal Charge (FC)
V = Valence Electrons
B = Bonding Electrons
N = Non Bonding Electrons
FC = V - 1/2(B) - N
Exceptions to the “octet rule” include some species having ____________ or _____________ octets
Incomplete or expanded octets
Delocalization involves electrons that are _______ by ________________ pair in a molecule/ion as opposed to being ______________ between _____________________ atoms
shared by more than one pair in a molecule/ion as opposed to being localized between a pair of atoms
Electron Geometry of 5 Bonding Pairs
Trigonal Bipyramidal
Electron Geometry of 6 Bonding Pairs
Octahedral
Molecular Geometry of 4 Bonding Pairs AND 1 Lone Pair
See saw
Molecular Geometry of 3 Bonding Pairs AND 2 Lone Pair
T-Shape
Molecular Geometry of 2 Bonding Pairs AND 3 Lone Pair
Linear
Molecular Geometry of 5 Bonding Pairs AND 1 Lone Pair
Square pyramidal
Molecular Geometry of 4 Bonding Pairs AND 2 Lone Pair
Square planar
A hybrid orbital results in the __________ of different types of orbitals on the _____________________
Mixing of different types of atomic orbitals on the same atom
Heat is a form of _____________
Energy
Temperature is a measure of the ___________________________________ of particles
Average kinetic energy
The Total Energy is _________________ in chemical reactions
The Standard State(Condition) is measured at _______
100kPa
The Enthalpy Change of Combustion
The enthalpy change when one mole of a substance is burnt in excess oxygen under standard conditions
The Enthalpy Change of Formation
The enthalpy change when one mole of a substance is formed from it’s elements under standard conditions
Using Hess’s Law, the equation for the enthalpy change of a reaction is =
Enthalpy change of products - Enthalpy change of reactants
Bond forming releases energy, which is ………
Exothermic
Bond breaking requires energy, which is ………
Endothermic
What is Ionization Energy? (Term)
The standard enthalpy change for the removal of one mole of electrons from one mole of gaseous atoms (or positively charged ions)
The Enthalpy of Atomization
The standard enthalpy change for the formation of one mole of separate gaseous atoms of an element in its standard state
What is Electron Affinity? (Term)
The standard enthalpy change for the addition of 1 mole of electrons by one mole of gaseous atoms of an element, to form one mole of gaseous ions under standard condition
Lattice Enthalpy
The standard enthalpy change for the formation of 1 mole of gaseous ions from the solid lattice
Enthalpy of Hydration
The standard enthalpy change for the addition of water to one mole of a gaseous ion to form a dilute solution
Enthalpy of Solution
The standard enthalpy change for when one mole of an ionic substance dissolves in sufficient water to form a dilute solution
Equation for Formation Enthalpy (Methane) (Standard States)
C(s) + 2H2(g) → CH4(g)
Equation for Lattice Enthalpy
MX(s) → M^+(g) + X^-(g)
Equation for Atomization
1/2X2(g) → X(g)
Equation for Ionization Energy (1st)
M(g) → M^+(g) + e^-
Equation for Hydration
M^+(g) → M^+(aq)
List the process for the Born Haber Cycle (Enthalpy of….)
Formation, Atomization, Ionization Energy, Electron Affinity, Lattice
Which Enthalpies in the Born Haber Cycle go Against the others (thus needs to be flipped)
Enthalpy of Formation and Lattice Enthalpy
Entropy refers to the ____________________________ among the particles
distribution of available energy
The state with the highest entropy
Gases
The rate of reaction is the…….
Change in concentration of a reactant or product over unit time
Note
Flashcard