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Chapter 1: Atoms
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- 1compositions of matterpure substance / mixture
- 2a pure substance can bean element or compound
- 3a mixture can beheterogeneous or homogeneous
- 4heterogeneouscomposition varies from one region of the mixture to another
- 5homogeneoushas the same composition throughout
- 6law of conservation of massin a chemical reaction, matter is neither created nor destroyed
- 7law of definite proportionsall samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements
- 8law of multiple proportionswhen 2 elements form 2 different compounds, the masses of element B that combine with 1g of element A, can be expressed as a ratio of small whole numbers
- 9law of multiple proportions examplecarbon monoxide / carbon dioxide
CO2 mass = 2.67
CO mass = 1.33
2.67 / 1.33 = 2
always divided the larger # by smaller # - 10nuclear theory- proposed by Ernest Rutherford
- most of the atoms' mass and all of its positive charge are contained in nucleus
- most of volume is empty; electrons are dispersed throughout
- # of electrons = # of protons - 11atomic number- given the symbol Z
- # of protons in nucleus - 12isotopes- atoms with the same number of protons but different numbers of neutrons
- generally exhibit the same chemical behavior - 13mass number- represented by the symbol A
- the sum of neutrons & protons - 14ions- during chemical changes, atoms can lose or gain electrons and become charged particles
- behave different than the atoms from which they are formed - 15for many elements, the (blank) is much more common than the (blank).- ion
- atom - 16cationspositively charged ions
- 17anionsnegatively charged ions
- 18true or false: the size of an isotope with more neutrons is larger than one w/fewer neutronsfalse
# of neutrons affects mass not size of atom - 19true or false: the size of an atom is the same for all of the element's isotopestrue
# of neutrons affects mass not size of atom - 20atomic massaverage mass of an element's isotopes, weighted according to the natural abundance of each isotope
- 21atomic mass formulaatomic mass =
(% of natural abundance * weight of isotope)
+ (% of natural abundance * weight of isotope) ... - 22mole (mol)- amount of material containing
6.02214 x 10^23 particles
- Avogadro's #
- amount of a substance
- value is = to the # of atoms in exactly 12g of pure carbon-12 - 23isoelectronichaving the same numbers of electrons
- 24alpha particle- + charged particle of a He nuclei
- composed of 2 protons/2 neutrons
- represented as a Helium-4 atom
- as it breaks away from nucleus it has no electrons, so it has a +2 charge - 25beta particlea fast-moving electron emitted by radioactive decay of substances
- 26isotopes of hydrogenDeuterium = one proton/neutron
protium = one proton/no neutrons - 27allotropetwo or more different physical forms in which an element can exist
i.e. graphite, charcoal, diamond are all allotropes of carbon - 28electropositivetend to lose electrons and form positive ions in chemical reactions
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- (Chem I) General Chemistry Fichas sobre Chapter 1: Atoms, creado por Alexandra Bozan el 28/12/2018.
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- Alexandra Bozan
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