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Section 1

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molar mass

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Chemistry Science

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Date created

Mar 1, 2020

Cards (18)

Section 1

(18 cards)

molar mass

Front

the mass of one mole of a pure substance

Back

Relative atomic mass

Front

mass of an atom relative to the Carbon-12 atom

Back

Modern Atomic Theory

Front

1. All matter is composed of atoms 2.atoms of any one element differ in properties from atoms of another element.

Back

Plum Pudding Model (who found it and what did it look like)

Front

J.J Thomson -Atoms are electrically neutral over all -Atoms contain electrons which are negatively charged -The mass of an electron is much less than mass of an atom Model: Electrons are spread throughout a positively charged positive space like seeds in a water melon (later disproved)

Back

Discovery of the Nucleus (who and how)

Front

Ernest Rutherford -Bombarded a piece of gold foil with possibility charged particles -Most particles went straight through the gold but some deflected away -Rutherford believed that the particles were hitting off positively charged spaces in the center of the atom called the nucleus.

Back

nuclear symbol

Front

the superscript indicates the mass number and the subscript indicates the atomic number

Back

mass number

Front

the sum of the number of neutrons and protons in an atomic nucleus

Back

atomic number

Front

the number of protons in the nucleus of an atom

Back

hyphen notation

Front

the mass number is written with a hyphen after the name of the element

Back

mole

Front

The amount of substance that contains as many particles as there are in exactly 12 grams of carbon in carbon-12

Back

Current Atomic Model (who and what)

Front

Rutherford Nucleus- Protons and neutrons held together by nuclear forces Electron cloud- Surrounds the Nucleus filled with electrons *all atomic nuclei contain protons and neutrons except for nuclei of most hydrogen atoms.

Back

law of definite proportions

Front

a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size

Back

Dalton's Atomic Theory

Front

1.All matter is composed of extremely small particles called atoms 2.Atoms of a given element are identical in size, mass and other properties 3. Atoms can not be subdivided created or destroyed 4.Atoms of different elements combine in simple whole number ratios. To form chemical compounds 5. In a chemical reaction atoms are combined, separated or re arranged

Back

Law of Multiple Proportions

Front

if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers

Back

Discovery of an electron (person and what he did)

Front

J.J Thomson Used a cathode ray tube to conduct his experiments. Passed a beam through a cathode ray tube and noticed it curved away from a positively charged piece of metal.

Back

average atomic mass

Front

the weighted average of the atomic masses of the naturally occurring isotopes of an element

Back

Isotope

Front

Atoms of the same element that have different numbers of neutrons

Back

Avogadro's number

Front

6.02 x 10^23

Back