CHEM 1150 Lecture Notes - Lecture 3: Iodate, Atomic Mass, Atomic Theory

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scarletbeetle212

27 Apr 2018

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3 laws that led to atomic theory:

Law of Conservation of Mass

Mass remains constant during a chemical reaction

Law of Definite Proportions

All samples of a given compound, regardless of their source or how

they were prepared, have the same proportions of elements

Mass ratio: mass of one element/ mass of second element

(larger divided by smaller)

□

Law of Multiple Proportions

When 2 elements (A and B) form 2 different compounds, the

masses of element B that combine w/ 1 g of element A can be

expressed a ratio of whole #s

Dalton's Atomic Theory:

Each element consists of tiny indestructible particles called atoms

Atoms of an element are identical in mass and other properties and are

different from atoms of any other element

Atoms combine in simple small number ratios to form compounds

Atomic theory today

An atom is defined by the number of protons it has

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Periodic table:

Atomic symbol: x

Atomic number (# of protons): z

Isotope symbols:

Isotopes: diff # of neutrons

□

Atomic mass: weighted avg via all naturally occurring isotopes

Ions: charged atoms (more or less electrons)

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Intro to bonding:

Covalent compounds

When share electrons

□

Usually b/w nonmetals

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Ionic compounds

Transfer of electrons from metals to non-metals

□

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Periodic table

Transition metals have varying oxidations

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Polyatomic ions: group of non-metals bond covalently w/ a non-neutral

charge (so their charge is positive or negative)

"Nick the Baby Camel ate an Icky Clam Supper in

Phoenix"

Nitrate NO3-

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Bromate BrO3-

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Carbonate CO32-

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Iodate IO3-

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Chlorate ClO3-

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Sulfate SO42-

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Phosphate PO43-

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# of constants in each word= # of oxygens in each

polyatomic anions (y counts as a consonant in this

case)

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# of vowels= # of negative charges

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Word "ate" will remind you that finding -ate

polyatomic ions

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The ones in red do not exist

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Add permanganate, MnO4-and chromate, CrO42- (and

dichromate Cr2O72-)

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Chapter 2

Wednesday, January 17, 2018

11:40 AM

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Related Questions

What are the main ideas in Dalton's atomic theory?

1- Atoms of one element cannot change into atoms of anotherelement.

2 - Atoms combine in simple, whole number ratios to formcompounds.

3 - Each element is composed oftiny, indestructible particles called atoms.

4 - Nuclear particles combine in simple, whole number ratios toform atoms.

5 - Each atom is composed of elements.

6 - All atoms of a given element have the same mass and otherproperties that distinguish them from the atoms of otherelements.

7 - Atoms of one element can change into atoms of anotherelement.

In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound:

(a) Calculate the mass of fluorine per gram of iodine in each compound. (b) How do the numbers in part (a) support the atomic theory?

b) When all three numbers are divided with 0.15, it gives: 5, 3, and 7. So, F and I form compounds in constant, whole number ratios. This is a law of multiple proportions and goes along with Dalton’s atomic theory since the F and I atoms combine in known ratios, and the masses of atoms are constant.