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57 Cards in this Set
- Front
- Back
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Physical Change (define)
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change in the physical appearance of the substance, but the particles are still the same
e.g. boiling water. H2O changes into a gas but the molecules are still H2O |
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Chemical Change (define)
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the molecules themselves are changed
e.g. separating H2O into 2H2 and O2 (using electricity) |
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visible properties (list some)
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transparent, translucent, opaque, clear, cloudy
colourless, red, yellow, black lustrous, dull, shiny liquid, solid, gas |
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behavior properties (list some)
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taste, texture, ductility, brittleness, odor, hardness, malleability, viscosity, conductivity
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Democritus
who was he what did he think/find explanation/model flaws |
a greek philosopher from 400 BC
there must be an indivisible particle called the atom they must be different sizes in constant motion empty spaces |
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John Dalton
who was he what did he think/find explanation/model flaws |
Scientist from 1807
same elements have the same atoms indivisible rearranged to form different substances cannot be created or destroyed does not explain why some repel/attract each other |
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J. J. Thomson
who was he what did he think/find explanation/model flaws |
Scientist of 1897
discovered electrons the rest of the atom must be positive evenly distributed throughout atom raisin bun models proved wrong later |
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Rutherford
who was he what did he think/find explanation/model flaws |
Scientist of 1909
tin foil experiment found that protons and electrons were not distributed evenly dense positive nucleus electrons circle nucleus bee-hive |
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Chadwick
who was he what did he think/find explanation/model flaws |
Rutherford's student in 1932
he discovered a particle with no charge that could disintegrate atoms with extreme power nucleus contains the neutron about same mass as proton |
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Bohr
who was he what did he think/find explanation/model flaws |
Scientist of 1913
Using the light experiment- different elements create different colors electrons have orbits that circle the nucleus. Their orbit is determined by its amount of energy Cannot exist between shells Each shell can hold a certain number of electrons |
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Molecules (define)
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compound of different elements/multiple atoms
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Translucent (define)
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cloudy/semi-transparent
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Exothermic (define)
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reaction gives off heat
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Endothermic (define)
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reaction absorbs heat
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Valence (define)
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out-most shell of the atom
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Stable (define)
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a stable atom has a full valence shell and is therefore not very reactive
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Octet rule (define)
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atoms will gain or lose electrons in a chemical reaction in order to achieve a full valence shell (and become stable)
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Ion (define)
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an atom that has a positive or negative charge (more or less electrons than protons)
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Cation (define)
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an atom that has a positive charge
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Anion (define)
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an atom that has a negative charge
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Isoelectronic (define)
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when an atom has the same electron configuration as another atom
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Isotopes (define)
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atoms with an unusual amount of neeutrons
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protium (define)
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most common atom for the element terms of neutron count
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deuterium (define)
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second most common atom for the element in terms of neutron count
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tritium (define)
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third most common atom for the element in terms of neutron count
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atomic mass (define)
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average atomic mass on periodic table. Is the average of all known isotopes.
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Compounds (define)
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particles made up of two or more elements that create a more stable substance
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How to count atoms
symbol subscript subscript outside bracket co-efficient |
symbol represents one atom of the element
subscript (lower right corner behind the symbol) indicates how many atoms of that element are in a molecule of the substance multiply subscripts and coefficients with everything inside the bracket |
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3 classifications for elements on the periodic table and where to find them
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metal- left of staircase except hydrogen
metalloid-staircase elements except aluminum non-metals-on the right of the staircase & hydrogen |
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Columns in the periodic table:
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Families/Groups. It determines how many valence electrons there are.
1A, 2A, 3A, 4A, 5A, 6A, 7A, 8A, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14, 15, 16, 17, 18 |
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Rows in a periodic table:
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Periods. It determines the number of shells.
1, 2, 3, 4, 5, 6, 7 |
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Parts of a periodic table
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Block A- Representative Elements
Block B- Transition / Inner Transition Elements |
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AMU
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Atomic Mass Units. Mass of one neutron or proton
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Family 1A/1
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Alkali metals. They react violently with water
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Family 7A/17
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Halogens. They react strongly with organic substances (disinfectants)
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Family 8A/18
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Noble gases. They are very stable and hard to trigger a reaction from.
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Rules for naming ionic compounds
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metal + non-metal
element + eleminide cation + anion |
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Elements are represented by ____ letters.
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3 letters. First is capital. Second or third are lower case.
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Family 2A/2
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Alkali Earth metals.
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Bohr-Rutherford Diagrams
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E.g.
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Lewis Diagrams
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E.g.
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The average atomic number is
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the average of all known isotopes of that element based on percent abundance.
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atomic number is
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the number that tells you how many protons are in that element
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Chemical Reactions happen when
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the new substance produced will be more stable than the original substance, which is achieved with a full valence shell.
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You represent a ion in a bohr-rutherford or lewis diagram by
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drawing brackets around with the new charge
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changing the number of neutrons will change/not change
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not change the charge
change the mass change the physical/chemical properties |
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changing the number of electrons will change/not change
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change the charge
not change the mass (enough to take into account) change the chemical/physical properties |
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Particle Theory (define)
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1. atoms are in constant motion
2. all matter is made of atoms 3. Particles attract each other 4. Particles move faster as the temperature increases 5. Different substances are made of different atoms` |
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Pure Substance (define & example)
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Substance made of only one kind of particle
Water |
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Mixtures (define and example)
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Substance made of at least two different types of particles.
Mechanical mixtures- cereal and milk Solutions- apple juice |
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Alloy (define and example)
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a solid solution of two or more metals
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Physical property (define)
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a characteristic of the substance that can be determined without changing the composition of the substance
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Qualitative property (define)
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a property of a substance that does not have a numerical value (e.g. taste, colour)
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Quantitative Property (define)
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a property of the substance that has a numerical value (e.g. density)
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Viscosity (define)
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the degree to which a fluid resists flow
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Physical change (define)
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a change where the composition of the substance remains unaltered and no new substance are produced
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Chemical change (define)
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a change in the starting substance or substances and the production of one or more new substances
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