Chemistry- Elements/compounds & Properties Of Matter

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Element

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A fundamental substance that cannot be broken down by chemical means to simpler substances. They are the BUILDING BLOCKS of all substances.

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Atom

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The smallest particle of an element.

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Symbols

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An abbreviation of an element.

(Ex of common elements: Al, Ba, B, Br, Ca, C, Cl, Co, Cu, F, Au, H, I, Fe, Pb, Li, Mg, Hg, Ne, Ni, N, O, P, K, Si, Ag, Na, S, Sn, Ti, Zn) (Found on the periodic table).

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Periodic Table: Groups

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Elements with similar chemical properties in columns (also known as families).

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Periodic Table: Noble Gases

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Elements that are all gases and nonreactive.

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Periodic Table: Alkali Metals (What group?)

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Group 1A

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Periodic Table: Alkali Earth Metals (What group?)

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Group 2A

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Periodic Table: Halogens (what group?)

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Group 7A

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Periodic Table: Transitional Elements

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Center of the periodic table.

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Metals

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Solid at room temperature (EXCEPT mercury), high luster, good conductors of heat/energy, malleable (hammered in sheets), and are ductile (drawn into wires). [Most have high melting point and high density].

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Nonmetals

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Not lustrous, low melting points, low density, and poor conductors of heat/energy. [Opposite of metals].

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Metalloids

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Properties that are between metal and nonmetal. (Semi-conductors).

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Diatomic Molecules

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Molecules that contain exactly TWO atoms.

(Ex: H2, N2, O2, F2, Cl2, Br2)

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Compounds

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A distinct substance that contains two or more elements chemically combined. (2 types: Molecular & Ionic).

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Molecule

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The smallest uncharged individual unit of a compound formed by the union of two or more atoms.

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Ion

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A positively or negatively charged atom(s).

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Cation

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Negatively charged ion.

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Anion

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Positively charged ion.

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Chemical Formula

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Shows the symbols and the ratio of the atoms of the elements in a compound.

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Subscripts

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Numbers that appear partially below the line and to the right of a symbol.

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Write the formula for the following compound:

Hydrogen Chloride: 1 atom hydrogen + 1 atom chlorine

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HCI

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Write the formula for the following compound:

Methane: 1 atom carbon + 4 atoms hydrogen

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CH4

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Write the formula for the following compound:

Glucose: 6 atoms carbon + 12 atoms hydrogen + 6 atoms oxygen

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C6H12O6

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Properties

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The characteristics of substances that give them their unique identities.

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Physical Properties

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A substance that can be determined without altering its composition (color, taste, odor, state of matter, density, melting point and/or boiling point).

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Chemical Properties

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The ability of a substance to form new substances either by reaction with other substances or by decomposition.

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Physical Changes

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Changes in physical properties (e.g. size, shape, and density).

(Ex: Sawing wood, boiling water, heating glass)

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Chemical Changes

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New substances are formed that have different properties and composition from the original.

(Ex: Forming copper (II) oxide from Copper (Cu) and Oxygen (O2), rusting of iron, boiling an egg, digesting food, burning wood).

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Reactants

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The starting substances (e.g. water, copper, and oxygen)

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Products

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The substances produced (e.g hydrogen, oxygen, and copper (II) oxide).

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Law of Conservation of Mass

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No change is observed in the total masses of the substances involved in a chemical change.

(Ex: Water (100g) ---> Hydrogen (11.2) + Oxygen (88.8g))
(100 g reactant | 100 g products)

*Mass of reactants = Mass of products*

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Law of Conservation of Energy

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Energy cannot be neither created nor destroyed.

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Energy

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The capacity of matter to do work

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Potential Energy (PE)

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Energy that an object has due to its position.

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Kinetic Energy (KE)

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Energy that matter has due to motion

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Joule/Calorie

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Quantity of heat energy

(4.184 joules (j) = 1 calorie (cal))

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Specific Heat

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Quantity of heat lost or gained require to change the temperature.

( (mass of substance) x (specific heat of substance) x (delta t (or temperature change) = heat)

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Calculate the specific heat of a solid in j/g°C and cal/g°C if 1638 J raises the temperature of 125 g of the solid from 25.0°C to 52.6°C

(Known: 125g solid, 52.6 - 25.0 = 27.6°C, heat= 1638 J)
*USE THE FORMULA*

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1638 J / 125g x 27.6°C = 0.475 J/g°C

-Convert joules to calories-

(0.475 J / g°C) x (1.000cal/ 4.184 J) = 0.114 cal/g°C

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A 110.0g sample of metal at 55.5°C raises the temp of 150.0g of water from 23.0°C to 25.5°C. Find the specific heat of the metal in J/g°C

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= 0.477 J/g°C

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Calculate the quantity of energy needed to heat 8.0g of water from 42.0°C to 45.0°C

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= 1.0 x 10 ^2 J

(or)

24 calories (cal)