Chemistry Unit Test Flashcards
Classifying substances
Pure substance: one type of particle
- element: one type of atom ex: Oxygen, God
- Compound: 2 types of atoms combined ex: H2O
Mixture: two or more particles
- Heterogenous: 2 or more visible phases
- Mechanical Mixture: separates by filtration, settling, Tyndall effect: pick up w/laser
- Suspension: sold in liquid sand in water
- Emulsion: Liquid in liquid ex: water and oil
- colloid: one substance suspended in other ex: milk not clear
Homogenous: having 1 visible phase
- Solution: particles dissolved together, can’t separate by Tyndall only distillation ex: salt water
Molecule Covalent bonding Molecular element Molecular Compound Properties SCSL
Molecule: 2 atoms held together by covalent bonding Covalent bonding: 2 atoms share a pair of electrons •molecular element: 2 or more SAME non metal joined by covalent bonding •molecular compound: 2 or more DIFFERENT non metals combine as pure substance •naming: use Greek #s Ex: dinitrogen •properties -soft, no conduct, form solution, low melting point
- Chemical reactions: GPEC
- Gas tests:
- Oxygen
- Hydrogen
- Carbon dioxide
- Water vapour: cobalt chloride
- forms gas, precipitate, energy change,colour change
- GAS TESTS
- Oxygen: reignites
- Hydrogen: pop sound
- Carbon dioxide: splint goes out/distinguish
- Water vapour: blue cobalt chloride paper turns pink
Conservation of mass
Mass of reactants=equals mass of products
Physical and chemical properties
•physical properties: Change is reversible like state, no new substance formed
-Chemical change: new substance formed w/different properties, impossible to reverse
Types of Chemical reactions
- Synthesis: two elements:compound join together producing bigger compound
- decomposition: breaking down the compound
- single displacement: element reacting with ionic compound element goes into compound the other element is by itself
- double displacement: two ionic compound switch places •combustion: element/ Compound react with oxygen producing water and carbon dioxide H2O CO2
Acids HCBrEMSS
Acid: compound dissolves in water producing hydrogen ions Properties: HCBrEMSS •hydrogen ion common •corrosive •blue litmus turns red, red stays red •electricity conducts •reacts with MAGNESIUM to produce hydrogen •sour taste, •reacts with sodium hydrogen carbonate to produce carbon dioxide Ex: vinegar
Base HEMBBrc
•compound that dissolves in water producing hydroxide -known as alkali and antacid •properties: •hydroxide ion common •electricity conduct •no reaction MAGNESIUM •bitter taste •blue litmus stay blue. Red turn blue •corrosive
Neutralization
Acid and base produced salt and water Ex: NaOH+HCl-> NACl+H2O
- formula: HB+XOH–>XB+H2O
pH scale
Acid- pH Less than 7 Base: higher than 7 to 14 Neutral: 7 Left= strong acid Right=strong base
Ionic compound SFCM
Ionic: it is a metal and non metal combined by 1 or more negative or positive charged ions Metal lose electron to non metal Transferring elections Conduct electricity
- properties: solid at room temp, form crystals, conduct electricity, ionic crystal attracts other ion crystal= high melting point
Polyatomic’s
Polyatomic’s: group of atoms of different elements acting as a single ion
Reading period of Table
Right 18= noble gases 17=halogens staircase b to Po= metallic On top of stair case C to Se: non metal Left 2: alkaline earth Left 1: alkali metal
How to create acid, base, neutralization
Acid: react non metal with oxygen to form non metal oxide, react the non metal with water to form acid Base: react metal with oxygen to form metal oxide than react with water to form base •neutralization: react acid and base to form salt and water
Combustion
Complete combustion: lots of Oxygen •carbon dioxide, water and energy is complete •is the hottest clearest flame Propane is complete combustion: C3H8 Propane+oxygen yields carbon dioxide+water+energy Incomplete: little oxygen •produces substances not carbon dioxide and water Produces: soot and carbon Soot black powder monoxide Carbon monoxide poisonous gas •has dirty colder yellow flame
