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Section 1

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chemical changes

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Chemistry Science

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Last updated

1 year ago

Date created

Mar 14, 2020

Cards (32)

Section 1

(32 cards)

chemical changes

Front

bubbles, color change, production of a solid, heat that is produced or absorbed

Back

oxidation-reduction reaction

Front

electrons are transferred from one substance to another

Back

avogradro's number

Front

6.02 x 10^23

Back

trigonal planar geometry

Front

120 degrees

Back

ion dipole forces

Front

- relatively stron electro static attractions between ions and polar molecules - causes the dissolution of the ionic solids in polar solvents such as water

Back

combination (synthesis) reactions

Front

-two or more elements form one product - simple compounds combine to form one product

Back

molar mass

Front

- the mass of 1 mole of an element - the average atomic mass expressed in grams

Back

the delta sign signifies...

Front

heat

Back

Linear geometry

Front

180 degrees

Back

To write a chemical reaction

Front

reactant 1 + reactant 2--> product 1 + product 2 starting material vs finishing material

Back

polar covalent bonds

Front

non metal atoms, unequal sharing of electrons, moderate electronegativity

Back

molar mass conversion factors

Front

- are fractions ( ratios) written from the molar mass - relate grams and moles of an element or compound

Back

diatomic molecules

Front

H2, N2, O2, F2, Cl2, Br2, I2

Back

polar molecules

Front

electrons shared unequally

Back

OIL RIG

Front

Oxidation Is Loss of Electrons Reduction Is Gain Electrons

Back

1 mole

Front

6.02 x 10^23

Back

equal bond electron sharing

Front

nonpolar bond unequal sharing of electrons = polar bond

Back

electronegativity

Front

of an atom is it's ability to attract the shared electrons in a bond - increases from left to right ( bottom to top) - low for metals - high for non metals

Back

non polar covalent bonds

Front

2 non metals, equal sharing, small electronegativity

Back

electronegativity numbers

Front

0-0.4 --> non polar 0.5-1.8--> polar greater than 1.8-> ionic

Back

single replacement reaction

Front

one element takes the place of a different element in another reacting compound

Back

double replacement reaction

Front

both ions in the reactant compounds switch places

Back

chemical reaction

Front

occurs when a substance is converted into one or more substances with different formulas and different properties

Back

subscripts in a formula

Front

- show the relationship of atoms in the formula - the moles of each element in 1 mole of a compound

Back

decomposition reaction

Front

- one substance splits ( or decomposes) into two or more simpler substances

Back

in a balanced equation

Front

- no atoms are lost or created ( conservation of matter) - the number of atoms on the reactant side is equal to the number of atoms on the product side

Back

VSEPR theory

Front

-describes the orientation of electron groups around the central atom - states that electron groups are arranged as far apart as possible around the central atom to minimize the repulsion between them - states that the specific shape of a molecule is determined by the number of atoms attached to the central atom

Back

double bond

Front

atoms share 2 pairs of electrons

Back

combustion reaction

Front

- carbon- hydrogen containing compound burns in oxygen gas to form carbon dioxide ( CO2) and water (H2O) - energy is released as a product in the form of heat

Back

tetrahedral geometry

Front

109 degrees

Back

non polar molecules

Front

bonding electrons are equally attracted to both bonded atoms

Back

triple bond

Front

atoms share 2 pairs of electrons

Back