atom: basic building blocks of matter structure: nucleus electron proton neutron
TRANSCRIPT
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Atom: basic building blocks of matterStructure:
Nucleus
Electron
Proton
Neutron
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Definitions: Nucleus- center of atom, contains
protons and neutrons Protons: positive charge (+) Neutrons: neutral charge (=)
Electrons- negative charge (-), orbit in energy levels on outside of atom
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Location of Subatomic Particles
nucleusProtons
Neutrons
electrons
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Energy Levels- Orbit around nucleus Forms “shells” around nucleus Electrons fill the shells from the inside
out
1st
3rd
2nd
N
1st level: max of 2 electrons
2nd level: max of 8 electrons
3rd level: max of 18 electrons
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Elements: all the same type of atoms bonded together Can’t be broken down into simpler
substances 90 occur naturally Others are man-made 25 essential to living organisms 99% of living organisms are made of
C,H,O,N
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Isotopes- atoms of the same element with different number of neutrons in the nucleus
Symbols- shorthand abbreviations for elements Rules:
First letter always capital Second letter always lower case Every element has a different
symbol Ex’s: Mg N O Na C Cl
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Periodic Table
Elements are arranged in columns known as a family or group
Families have similar properties because the outer shell of the atoms have the same number of electrons
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Atomic Mass on the Periodic Table
11
Na
22.99
Atomic Number
Symbol
Atomic Mass
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Atomic Number & Mass Meanings
Atomic number = the number of protons and the number of electrons (this will be equal for stable elements.)
Atomic mass – the atomic number = the number of neutrons (round to whole number)
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Molecule/Compound: a substance that contains different elements bonded together
Formula- a set of symbols that show the type of elements and the ratio in which they combine Ex’s: CO2 H2O
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Subscript- number after element indicating the number of atoms present
Coefficient- number in front of the formula indicating the number of molecules present Ex’s: 3H2O – 3 molecules of water
6NH4 – 6 molecules of ammonia
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Water: (H2O)
One of the most important compounds in living organisms
Makes up 70-95% of most organisms
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Properties of Water
1. Polar Molecule: it has an unequal distribution of charge. The oxygen side has a slightly negative charge, so ionic compounds dissolve easily in water.
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2. Resists temperature change
3. Expands when it freezes
4. High surface tension because the polar molecules are attracted to each other and form a slight film on the surface.
5. Capillary action, which means, plants can carry water up thin tubes.
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Organic & Inorganic Molecules
Organic molecules- contain carbon (C) Inorganic molecules- do not contain C
Which of the following are organic?
H2O NaCl C6H12O6 CaCO3
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Living Organisms are made up of 4 abundant and 9 less abundant elements:
C Hopkins café Magic Salt (NaCl)
*C= carbon Ca= calcium
*H= hydrogen Fe= iron
*O= oxygen Mg= magnesium
P= phosphorus Na= sodium
K= potassium Cl= chlorine
I= iodine
*N= nitrogen *makes up 99.3% of a
S= sulfur living organism
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Bonding
Covalent bond- chemical bond when two atoms combine sharing electrons
- Examples: sugars, fats, & proteins
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Ionic bond- bond formed by the mutual attraction of two ions of opposite charge Examples: salt (NaCl) Na+ Cl-
Hydrogen bond- electrical attraction between a slightly negative atom and a slightly positive atom. Very weak so molecules must be close to experience this attraction.
Examples: water (H2O)
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Chemical Equations
Reactants- substances that undergo a chemical reaction
Products- substances formed by the chemical reaction
*Chemical equations must be written so they are balanced! Atoms are neither created nor destroyed during chemical reactions.