Flashcards
science~chemistry
Cards in this deck (129)
- 1what are qualitative propertiesProperties of a substance that are not measured and do not have a numerical value. Can be described as colour, odour, and texture.
- 2examples of qualitative properties-the red car is shiny
-vinegar has a strong odour
-the paper is thin and white - 3what are quantitative propertiesA property of a substance that is measured and has a numerical value. Can be described by temperature, height and mass.
- 4examples of quantitative properties-The bike has a mass of 10 kg and is 2.0 m long
Todays temperature is one degrees Celsius - 5Define physical propertyA characteristic of a substance that can be determined WITHOUT changing the composition of that substance.
- 6How can you describe physical property*use your five senses*
(touch, taste, sight, sound, smell)
-colour, odour, bitterness, sweetness, malleability, boiling point, etc. - 7examples of physical properties-The chrome on the car is shiny
-The density of water is about 1.00 g/ml - 8what is a chemical propertya characteristic of a substance that is determined when the composition of the substance is changed and one or more NEW SUBSTANCES are produced.
- 9examples of chemical properties-Baking soda causes cake to rise
-we use chemicals to unclog shower heads - 10what is a chemical changeA change in the starting substance or substances and the production of one or more new substances.
- 11examples of chemical change-burning paper
-iron reacts with oxygen
-colourless egg whites turn white while cooking
-baking soda/vinegar reaction - 12evidence that a chemical change has happened-change in colour
-change in odour
-bubbles visible and not caused by heating (new substance in gas form produced)
-change in temp. or light
-new solid is seen - 13what is a physical changeA change in which the composition of a substance remains unaltered.
- 14examples of physical properties-folding paper into origami
-freezing water to ice
-cutting paper
-cracking an egg
-sugar dissolves - 15what is densityA measure of how much mass is contained in a given unit volume of a substance.
- 16how can density be calculateddivide the mass of a simple by it's volume
- 17what is volumeThe amount of space that a substance or object occupies.
- 18how to calculate volumedivide the mass of the object/substance by its density.
- 19what is massA measurement of how much matter is in an object
- 20how to calculate massmultiplying the density and volume of the object/substance
- 21what is the meniscusthe curve in the upper surface of liquid close to the surface of an object. can either be convex or concave
- 22how to measure meniscusread the centre of the meniscus line
- 23what is lengthA measure of how long something is
- 24example of lengthThe bike is 2.0 m long
- 25example of densitywater is heavier than oil it has a density of 1.0 g/ml while oil has a density of 0.8 g/ml
- 26example of massthe mass of the soda can is 390 g
- 27example of volumethe volume of a can of coke in 12 fluid ounces.
- 28what are the general lab safety rules (12)-Wear safety googles at ALL times
-Wear close toes shoes and long pants
-Long hair tied back
-no eating and drinking in the lab
-No fooling around lab equipment
-know the rules and regulations of the lab
-Always wash your hands after
-Turn of all electrical equipment when done
Learn where safety/first aid is
-Notify teacher when accident occurs (chemical spill, etc.)
-Read the label on chemicals twice before use
-If chemicals come in contact with eyes/skin flush with water immediately
ALWAYS BE CAREFUL - 29what are characteristic physical propertiesEither a physical or chemical property that is unique to a particular substance. Always the same whether comparing different sizes of the substance.
- 30what is an example and non-example of characteristic propertiesexample: the freezing point for water is -32 degrees celsius
non-example: the mass of a certain object like gold - 31what are some main characteristic properties help describe a substance. (6)-magnetism
-solubility
-freezing point
-melting point
-boiling point
-density - 32what are the four states of matter-solid
-liquid
-gas
-plasma - 33describe solidParticles of a substance form a solid when these forces of attraction are strong enough to hold the particles close together in a rigid shape
- 34describe liquidWhen heated, the particles gain energy and begin moving faster. Once gaining enough thermal energy, particles start sliding past each other. Attraction can no longer hold them together causing liquid state
- 35describe gasIf heating continues from liquid state the particles gain so much energy that they fall apart completely now causing gaseous state. they have very little force of attraction.
- 36summarize and define particle theory (5)Particle theory is a theory that describes the composition and behaviour of matter.
1. All matter is made up of tiny particles that have empty spaces between them
2. Different substances are made up of different kinds of particles.
3. Particles are in constant random motion.
4. The particles of a substance move faster as temperature increases.
5. Particles attract each other - 37what is matterMatter is anything that has mass and takes up space
- 38pure substanceA substance that is made up of only one type of particle
- 39mixtureA substance that is made up of at least two different types of particles
- 40mechanical mixtureA mixture in which you can distinguish between different types of matter
- 41solutionA uniform mixture of two or more subtances
- 42alloyA solid solution of two or more metals
example "solder" is tin and lead combined - 43heterogeneous mixturemade up of different substances that rain physically separate
- 44example of heterogeneous mixturesugar and sand
they are not completely mixed in together therefore called a heterogeneous mixture - 45homogeneous mixtureA mixture which has uniform composition and properties throughout
- 46example of homogeneous mixture-salt dissolved in water
-air (homogeneous mixture of gases) - 47what are all the changes of state (5)freezing
melting
condensation
evaporation
sublimation - 48what does a physical state in which a substance exists depend ontemperature
- 49describe freezing stateliquid-solid
needs to get colder - 50describe melting statesolid-liquid
needs to get hotter - 51describe condensationgas-liquid
needs to get colder
warm air hits cold surface - 52describe evaporationliquid-gas
needs to get hotter
can also be called boiling - 53describe sublimationeither:
gas-solid (cold)
or
solid-gas (hot)
can also be caused by atmospheric pressure - 54what is freezing pointThe temp. at which a substance changes state from a liquid to a solid
- 55melting pointThe temp. at which a substance changes state from a solid to a liquid
- 56boiling pointThe temp. at which a substance changes state rapidly from a liquid to gas
- 57controlled experimentAn experiment in which the independent variable is purposely changed to find out what change, if any, occurs in the dependent variable
- 58dependent variableA variable that changes in response to the change in the independent variable
- 59compoundA pure substance composed of two or more different elements that are chemically joined
- 60independent variableA variable that is changed by the investigator
- 61variableany condition that changes or varies the outcome of a scientific inquiry
- 62define and give an example of elementA pure substance that cannot be broken down into a simpler chemical substance by any physical or chemical means
example: helium He - 63define atomthe smallest unit of an element
- 64electron proton neutronelectron- A negatively charged particle found floating around the nucleus inside the atom
symbol: e-
Proton- A positively charged particle found in the nucleus of an atom
the symbol: p+
Neutron- A neutral particle in the atoms nucleus.
symbol: nº
- 65Atomic numberThe number of protons in an atom's nucleus
- 66mass numberThe number of protons and neutrons in an atom's nucleus
- 67isotopeAn atom with the same number of protons but different number of neutrons
- 68atomic massthe mass of an atom in atomic mass units
- 69element symbolAn abbreviation for a chemical element
- 70who created the periodic tableDmitri Mendeleev
- 71how to find electrons and protonslook for the atomic numbers on the elements of the periodic table. This atomic number will correspond to both the number of electrons and the number of protons in the atom.
- 72how to find neutronstake the atomic mass and subtract it by the atomic number to find the number of neutrons
- 73metalAn element found on the left side of the periodic table that is lustrous, malleable, ductile, and conducts heat and electricity.
- 74properties of metalsshiny
lustre
malleable
ductile
good conductor of heat and electricity - 75examples of metalsgold
copper
silver
iron
aluminum - 76define non-metalelements of the right side of the periodic table that is usually a gas, or a dull powdery solid, that does not conduct heat or electricity
- 77non-metal propertiesgases at room temperature
when in solid form, it's not shiny, malleable or ductile
brittle/shatters easily
not a good conductor of heat and electricity - 78examples of non-metalscharcoal briquette
oxygen
hydrogen
nitrogen - 79define metalloidsElements found in the middle of metals and non-metals that have properties of both metals and non-metals
- 80examples of metalloidsboron
silicon
germanium
arsenic
antimony
tellurium
polonium - 81alkali metalsfound in Group 1
elements-Lithium, Sodium, Potassium
shiny, silvery, soft, highly reactive, low densities, can float on water - 82Alkaline Earth metalsGroup 2
Beryllium, magnesium, Calcium, Strontium, Barium, Radium
Shiny, silvery, not as soft/reactive as alkali metals, burn with bright colourful flames - 83Noble GasesGroup 18
stable nature of elements
low density-Helium
Neon used for signs
colourless, odourless, tasteless
glow brightly when electrical currents are passed through them
Argon-glows blue
Krypton-pink
Xenon-purple
non-toxic - 84HalogensGroup 17
Fluorine, Chlorine, gases at room temperature at atmospheric pressure.
Bromine-liquid
Iodine-astsatine solid
very reactive
poisonous in large amounts
some like Chlorine toxic in small amounts - 85How are elements arranged on the periodic tableby increasing mass
lightest to heaviest - 86Oxygen familyGroup 16
also called chalcogens
consists of oxygen, sulphur, selenium, tellurium, polonium - 87nitrogen familyGroup 15
nitrogen, phosphorus, Arsenic, Antimony, Bismuth - 88Carbon familyGroup 14
carbon, Silicon, Germanium, Tin, lead - 89Boron familyGroup 13
Boron, Aluminum, Gallium, Indium, Thallium - 90transition metalsFound in Groups 3-12
malleable, ductile, conduct energy and heat
some are
iron, cobalt, nickel, copper, zinc, scandium, titanium, vanadium, Chromium, manganese, silver etc. - 91moleculegroup of two or more atoms chemically joined
- 92how do you find the number of atoms in a molecule (H2O)2-hydrogen
1-Oxygen - 93reactantA substance that takes part in or undergoes change during the reaction
- 94productSubstances formed during the chemical reaction
- 95yieldAlso called reaction yield
Amount of product contained in the chemical reaction - 96CatalystA substance that speeds up the chemical reaction but is not consumed by the reaction.
- 97Writing a chemical word equationtake two elements (iron and oxygen)
*make sure the first element is metal and second non-metal*
+2 -2
Fe O
Cross over numbers now they have both ions of two.
same number ions take each other out and 1's are taken out as well.
therefore this is
FeO
or
Iron Oxide - 98—bunsen burner
- 99—beaker
- 100—Erlenmeyor flask
- 101—test tube
- 102—thermometer
- 103—eye dropper
- 104—clay triangle
- 105—funnel
- 106—mortar and pestle
- 107—ring clamp
- 108—retort stand
- 109—graduated cylinder
- 110lanthanide seriesA group of elements from periods 57-71 on the periodic table
- 111actinide seriesA series of 15 radioactive elements with increasing atomic numbers from actinium to lawrencium
- 112What are the rules of metric1. Number, space, unit
example: 70 cm (not 70cm)
2. No periods
example: 1.36 m (not 1.36 m.)
3. Numbers and symbols together
example: 6 m or six metres (not 6 metres or six m)
4. Decimal fractions not common fractions
example: 0.25 m (not 1/4 m)
5. A zero is placed before the decimal marker
example: 0.1 m (not .1 m)
6. spaces separate groups of 3 digits on either side of the decimal point and numbers of four digits is not separated into groups of three
example : 340 456 000
or
3400 - 113—crucible
- 114—safety goggles
- 115—hot plate
- 116—test tube holder
- 117—test tube clamp
- 118—rubber stopper
- 119—glass plate
- 120—test tube cleaner
- 121—wire mesh
- 122—flint
- 123—crucible tongs
- 124—glass bottle
- 125—scoopula
used to scoops and transfer chemicals
- 126—forceps
- 127—depression slide
comparing small amount of chemicals
- 128—glass rod
for stirring
- 129—overflow can
used with a graduated cylinder for measuring volume of odd shaped objects
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- these are flash cards to better understand chemistry
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- time4me
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