CHEM 1210 Study Guide - Summer 2018, Comprehensive Midterm Notes - Ion, Ultraviolet, Oxygen
CHEM 1210
MIDTERM EXAM
STUDY GUIDE
Fall 2018
CHEM 1210
CHAPTER ONE…
Pure Substance
Made up of only one type of particle with invariant composition
Mixture
A substance composed of two or more particles in proportions that can vary from one
sample to another
Element
A substance that cannot be chemically broken down into simpler substances
Compound
A substance composed of two or more elements in fixed, definite proportions
Heterogeneous Mixture
A mixture in which the composition varies from one region of the mixture to another,
the particles do not mix uniformly
Homogeneous Mixture
A mixture with the same composition throughout
John Dalton (1766-1844)
Proposed the atomic theory
Law of Conservation of Mass
In a chemical reaction, matter is neither created nor destroyed
Law of Definite Proportions
All samples of a given compound, regardless of their source or how they were
prepared, have the same proportions of their constituent elements
Law of Multiple Proportions
When two elements form two different compounds, the masses of element B that
combine with 1 g of element A can be expressed as a ratio of small whole numbers
Atomic Theory
1: Each element is composed of tiny, indestructible particles called atoms
2: All atoms of a given element have the same mass and other properties that
distinguish them from the atoms of other elements
3: Atoms combine in simple, whole-number ratios to form compounds.
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4: Atoms of one element cannot change into atoms of another element. In a chemical
reaction, atoms only change the way that they are bound together with other atoms
J.J. Thomson (1856-1940)
Cathode Ray Experiment- discovered the electron. Plum pudding model
Robert Millikan (1868-1953)
Oil Drop Experiment- found the fundamental charge of a single electron and mass of
an electron from that. Charge: -1.60 X 10^-19 C. Mass: 9.10 X 10^-28 g
Ernest Rutherford (1871-1937)
Gold Foil Experiment- formed nuclear theory
Nuclear Theory
1: Most of the atom's mass and all of its positive charge are contained in a small core
called the nucleus.
2: Most of the volume of the atom is empty space, throughout which tiny, negatively
charged electrons are dispersed.
3: There are as many negatively charged electrons outside the nucleus as there are
positively charged particles (named protons) within the nucleus, so that the atom is
electrically neutral.
Atomic Number
The number of protons in an atom's nucleus, given by the symbol Z.
Chemical Symbol
A one or two letter abbreviation for an element, given by the symbol X.
Mass Number
The sum of the number of neutrons and protons in an atom, given by the symbol A.
Isotopes
Atoms with the same number of protons but different numbers of neutrons
Ions
An element with a positive or negative charge created through a chemical change
when gaining or losing an electron
Cations
Positively charged ions
Anions
Negatively charged ions
Atomic Mass
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Document Summary
Made up of only one type of particle with invariant composition. A substance composed of two or more particles in proportions that can vary from one sample to another. A substance that cannot be chemically broken down into simpler substances. A substance composed of two or more elements in fixed, definite proportions. A mixture in which the composition varies from one region of the mixture to another, the particles do not mix uniformly. In a chemical reaction, matter is neither created nor destroyed. All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. When two elements form two different compounds, the masses of element b that combine with 1 g of element a can be expressed as a ratio of small whole numbers. 1: each element is composed of tiny, indestructible particles called atoms.
