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| example of qualitative observation |
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| example of quantitative observation |
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3" pencil
quantity observation |
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| a set of hypothesis that gives an overall explanation of some part of nature |
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| generally observed behaviors summarized into a statement |
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| fundamental unit of which elements are composed |
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| _________tells what happens and _________ is our attempt to explain why it happens |
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| the law of constant composition applies to________ |
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| the fundamental particle according to Dalton |
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| The 1st scientist to show that atoms emit tiny negative particles |
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| the tiny negative particles |
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| which atomic particle determines the chemical behavior of an atom |
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| The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus of an atom contains a dense center of positive charge |
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| what 2 scientist discovered the neutron |
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| James Chadwick and Ernest Rutheford |
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| atoms with same # of protons but different # of neutrons |
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| the # of protons in the nucleus of an atom |
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non metal
alkali metal
alkali earth metal
noble gas
halogen
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| elements right next to stair step like in periodic table |
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| lanthanides and actinides are periods also called |
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| different form of a given element |
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The normal chemical symbol is used for the isotope with the addition of the atomic number (Z) at the lower left of the symbol and the atomic mass number (A) at the upper left as shown [image]X.
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| who is given the credit for the developing the periodic table of elements |
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Definition
1. Write the name of the element represented by the first symbol in the formula.
2. Write the name of the element represented by the second symbol in the formula, but change the ending of the element's name to "ide".
3. Check a reference table to determine the number of positive oxidation numbers that the first element forms. If it only forms one then you are done.
4. If the first element shows more than one oxidation number, than use the stock system. Determine the oxidation number that the first element is showing and write that roman numeral in-between the two elemental names.
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| Rules for Naming Acids that Do Not Contain Oxygen in the Anion: |
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Definition
- Since all these acids have the same cation, H+, we don't need to name the cation.
- The acid name comes from the root name of the anion name.
- The prefix hydro- and the suffix -ic are then added to the root name of the anion.
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| Rules for Naming Oxyacids (anion contains the element oxygen) |
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Definition
- Since all these acids have the same cation, H+, we don't need to name the cation.
- The acid name comes from the root name of the oxyanion name or the central element of the oxyanion.
- Suffixes are used based on the ending of the original name of the oxyanion. If the name of the polyatomic anion ended with -ate, change it to -ic for the acid and if it ended with -ite, change it to -ous in the acid.
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| Naming Polyatomic compounds |
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Definition
The cation is written first in the name; the anion is written second in the name.
Rule 2. When the formula unit contains two or more of the samepolyatomic ion, that ion is written in parentheses with the subscript written outside the parentheses.
Note: parentheses and a subscript are not used unless more than one of a polyatomic ion is present in the formula unit (e.g., the formula unit for calcium sulfate is "CaSO4" not "Ca(SO4)").
Rule 3. If the cation is a metal ion with a fixed charge, the name of the cation is the same as the (neutral) element from which it is derived (e.g., Na+ = "sodium"). If the cation is a metal ion with a variable charge, the charge on the cation is indicated using a Roman numeral, in parentheses, immediately following the name of the cation (e.g., Fe3+ = "iron(III)").
Rule 4. If the anion is a monatomic ion, the anion is named by adding the suffix -ide to the root of the element name (e.g., I- = "iodide"). |
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the measure of the attraction of an atom for the electrons in chemical bond
----increases
l
decreases |
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energy required to completely remove an electron from an atom or ion
-----decrease
l
increase |
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| how to determine p/e/n in ions |
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Definition
p remains the same
n remains the same
e changes according to number
+ = subtract
- = add |
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| A sample of matter, either an element or a compound, that consists of only one component with definite physical and chemical properties and a definite composition. |
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C and c
physical and chemical properties |
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Definition
| Physical properties are charecteristics of a pure substance that can be observed without changing it into another substance. Chemical properties are charecteristics of a pure substance that describes its ability to change into different substance. |
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c and c
physical and chemical change |
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Definition
A chemical property is a characteristic of a substance that is observed when it undergoes a chemical change.
1) Physical properties are properties of an element or compound that can be observed without a chemical reaction of the substance. Density and electrical conductivity are examples of physical properties. |
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Definition
Solids - Keep their shape
Definite mass ( will not change in size )
Definite volume ( will not change shape )
High melting point
Molecules vibrate slowly in place |
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Definition
Liquids - Take shape of container
Definite mass
Indefinite volume ( will change in shape under certain conditions )
Molecules vibrate rapidly and freely |
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Gases - Take shape of container and fill completely
Indefinite mass and volume
Expand rapidly and evenly to fill container
When released in large area ( class room, outside, outer space, ) will fill entire area and become extremely scarce. |
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