Review Flashcards
Define quantitative property
these are the measured properties involving #’s and units
Define the term qualitative property
description or characteristics about substance using senses
Describe where metals are
Left of the staircase
Describe where non-metals are
Right of the staircase
Describe where metalloids are
Stairs
Describe physical change
changes that occur in shape,form,appearence or state. No new substance is formed
Describe Chemical change
One or more new substances form in a reaction
What are chemical change clues
C- colour changed H-heat,light,sound I-irreversible P-percipitate ( soild, tiny flecks, thickening) \+ G- gas formation (smoke, bubbles) & order change
What is matter divided into
Pure stubstance, and Mixtures
What are pure substance divided into
Elements and Compounds
What are mixtures divided into
Heterogenous, and Homogenous
What is an observation
recording what happened durning a lab using your senses
What is inferences
take observations and use prior knowledge to explain it
Dalton
element exist as uncuttleable particle, thought charge less spheres
Thomson
discovered the electron
cathode-ray tube experiment
Rutherford
Nucleus’s, densely positive, electrons move, gold foil experiment, atom made of empty space
Chadwick
Neutrons found in nucleus
Bohr
Electrons orbit nucleus’s at set speed and energy level
What is a Ion
a stable ion, an atom becomes stable by gaining or loosing electrons
Caton
Have positive charges, these atom lost electrons and therefore metals
Anion
Have negative charges, atom has gained electrons, non metals
Isotopes
Atoms of an element that share the same number of electrons and proton but differ in mass. The neutrons
Average atomic mass equation
Mass isotope x abundance + Mass isotope x abundance…
What are the 4 types of Orbitals?
S orbitals
P orbitals
D orbitals
F orbitals
S orbitals
Spherical shape, made of 1 su shell which can hold 2 electrons max
P orbitals
Dumbbell in shape (3), made up of 3 su shells, hold up to 6 electron max
D orbitals
Dumbbell In shape 5, made up of 5 subshells, can hold ten electrons max
F orbitals
Dumbbell in shape (7), made up of 7 subshells and can hold up to 14 electrons max
Electron configuration
Electrons get filled from lowest energy orbitals onwards. 1S is lowest orbital.
Condensed Electron Configuration
Select last noble has that was passed through when deciding E.C looked like for the element
Place symbol in bracket
Then write only remaining E.C
Fluorine [He] 2S2 2P5
Energy Level Diagram Rules
Hund’s Rule— each subshells within an orbital must have 1 electron in each position
Aufbaus rule- electrons must fill lower energy levels first
Ionic Compounds Properties
- made up of 1 metal and 1 or more non metals
- metals appear first
- form crystal lattice structures-lots of bonds holding crystal together
- soild at room temperature
- soluble in water
- form electrolytes
- provide path for electrons to form on therefore are good conductors of heat and electricity (as a solution)
- melting boiling point high due to the increased energy needed to break down crystal bonds
Formation of Ionic Bonds
Gain or loose electrons to become stable
3 step symbols
Draw Lewis Symbol for each element
Show the ions ( gain and loose e)
Show chemical formula
What is an Ionic Bond
The electrostatic force of attraction between ion+ and ion-
Formula unit
The smallest repeating unit in an ionic crystal
Electrolyte
A compound that dissolves in water producing a solution that conducts electricity
Ionic Compounds with Binary Metals
Metal found in group 1 and 2 + Al,Zn,Ag All have 1 ionic charge
Metals appear first and name doesn’t change
Non metal name changes to ide
Ionic Compounds with Multivalent Metals
Metals found in group 3 all the way to the staircase
2 naming systems
Stock
Classical
Stock Naming System
Involves using Roman numerals to represent the ionic charge for metals
Always go with most common when haven’t been told
Metal keeps name followed by Roman numerals
Non metals change to ide
Classical Naming System
Identifies ionic charge for metals using a suffix on the end of metals name
Ic for the higher value
Ous for lower
All transition metals use this except the ones with one charge
Metals change to ide
Latin Root names
Iron:Ferrum Copper:Cuprum Tin:Stannum Lead:Plumbum Gold:Aurum
Polyatomic Ions
are usually anion units meaning they have a common charge for 2 or more combined non metals
Majority are called (oxyanions) because they have oxygen in the unit
Metals keep name if binary or multivalent
Non metal change to ate or ite if looses oxygen
Exceptions apply
6 Polyatomic Ions
Hydroxide - (OH)-1 Chlorate-(ClO3)-1 Nitrate-(NO3)-1 Sulfate-(SO4)-2 Carbonate(CO3)-2 Phosphate(PO4)-3
