Chapter 2 Atoms, Molecules, And Ions

Front 1

Dalton's atomic theory shows several laws

Back 1

law of constant composition: the relative nubers and kinds of atoms are constant.
law of conservation of mass: the total mass of materials present after a chemical reaction is the same as the total mass present before the reaction.
law of multiple proportions: if two elements A and B combine to form more than one compound, the masses of B that can combine with a given mass of A are in the ratio of small whole numbers

Front 2

Dalton's Atomic theory

Back 2

-Each element is composed of extremely small particles called atoms
-All atoms of a given element are identical, but the atoms of one element are different from the atoms of all other elements.
-Atoms of one element cant be changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions.
-Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms.

Front 3

Atoms are composed of

Back 3

subatomic particles: electrically charged particles

Front 4

true or false:
Particles with the same charge repel one another and particles with unlike charges attract one another

Back 4

True

Front 5

J.J. Thomson created the....

Back 5

plum pudding model which proposed that the atom consisted of a uniform positive sphere of matter in which the electrons were embedded like raisins in pudding.

Front 6

Who discovered protons and the nucleus of the atom and proved Thomson wrong?

Back 6

Rutherford. He found that the volume of an atom is empty space in which electrons move around the nucleus.

Front 7

what is the charge of an electron

Back 7

1-

Front 8

what is the charge of a proton

Back 8

1+

Front 9

what is the charge of a neutron

Back 9

It is electrically neutral.

Front 10

true or false: every atom has an equal number of electrons and protons, so atoms have no net electrical charge.

Back 10

true

Front 11

true or false: electrons take up most of the atoms volume

Back 11

true

Front 12

the ____ contains most of the mass of an atom

Back 12

nucleus

Front 13

amu of proton, neutron, and electron

Back 13

1.0073, 1.0087, 5.486 x 10^-4

Front 14

what makes an atom of one element different from an atom of another element?

Back 14

they have a different number of protons or atomic number

Front 15

what are isotopes?

Back 15

Atoms with identical atomic numbers but different mass numbers...so different amount of neutrons

Front 16

what are the horizontal rows of the periodic table

Back 16

periods

Front 17

what are the vertical rows of the periodic table

Back 17

groups

Front 18

Elements in the same _____ have similar properties because they have the same arrangement of electrons in their atoms.

Back 18

group

Front 19

properties of metallic elements or metals

Back 19

-luster
-high electrical and heat conductivity
except for mercury Hg, they are solid at room temperature
-does not include hydrogen

Front 20

Is hydrogen a metal, nonmetal or metalloid?

Back 20

nonmetal

Front 21

what are metalloids

Back 21

elements that share both properties of metals and nonmetals

Front 22

Alkali metals

Back 22

group 1A
Lithium, Sodium, Potassium, Rubidium, Caesium, Francium

Front 23

Alkaline earth metals

Back 23

Group 2A
Beryllium, Magnesium, Calcium, Strontium, Barium, Radium

Front 24

Chalcogens

Back 24

Group 6A
Oxygen, Sulfur, Selenium, Tellurium, Polonium

Front 25

Halogens

Back 25

Group 7A
Fluorine, Chlorine, Bromine, Iodine, Astatine

Front 26

Noble gases

Back 26

Helium, Neon, Argon, Krypton, Xenon, Radon

Front 27

what is a diatomic molecule?

Back 27

a molecule made up of two atoms.

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

Front 28

what are molecular compounds?

Back 28

compounds composed of molecules that contain more than one type of atom.
Ex: CH4, methane.

Front 29

Molecular formula vs. empirical formula

Back 29

molecular formula: chemical formulas that indicate the actual numbers of atoms in a molecule
Ex: hydrogen peroxide H2O2

empirical formula: chemical formulas that show subscripts that are always the smallest possible whole-number ratios
Ex: hydrogen peroxide HO

Front 30

true or false: if we know the empirical formula its obvious what the molecular formula is

Back 30

false. if we know the molecular formula of a compound, we can determine its empirical formula.

Front 31

what is an ion

Back 31

when electrons are removed from or added to an atom.
cation-positive charge
anion-negative charge

Front 32

what is an ionic compound

Back 32

a compound made up of cations and anions (metals and nonmetals).

Front 33

true or false: molecular compounds are mainly made of nonmetals only

Back 33

true