Lesson 2

Question 1

Who championed the theory that atoms are the fundamental building blocks of matter that reemerged the in the early nineteenth century?

Answer 1

John Dalton

Question 2

Each element is composed of extremely small particles called atoms.

Answer 2

Atomic Theory of Matter p.1

Question 3

All atoms of a given elements are identical, but the atoms of one element are different from the atoms of all other elements.

Answer 3

Atomic Theory of Matter p.2

Question 4

Atoms of one element cannot be changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions.

Answer 4

Atomic Theory of Matter p.3

Question 5

Compounds are formed when atoms are more than one element combine; a given compound always has the same relative number and kind of atoms.

Answer 5

Atomic Theory of Matter p.4

Question 6

Each element is composed of extremely small particles called?

Answer 6

Atom

Question 7

The total mass of substances present at the end of a chemical process is the same as the mass of substances present before the process took place.

Answer 7

Law of Conservation of Mass states

Question 8

This law was one of the laws on which Dalton’s atomic theory was based.

Answer 8

Law of Conservation of Mass

Question 9

If two elements, A and B, form more than one compound, the masses of B that combine with a given mass of A are the ratio of small whole numbers.

Answer 9

Law of Multiple Proportions

Question 10

Dalton predicted this law and observed it while developing his atomic theory.

Answer 10

Law of Multiple Proportions

Question 11

When two or more compounds exist from the same elements, they can not have the same relative number of atom.

Answer 11

Law of Multiple Proportions

Question 12

In Dalton’s view, the atom was the smallest particle possible. Many discoveries led to the fact that the atom itself was made up of smaller particles.

Answer 12

Discovery of Subatomic Particles

Question 13

Electrons and cathode rays; radioactivity; nucleus, protons, and neutron

Answer 13

Discovery of Subatomic Particles

Question 14

Streams of negatively charged particles were found to emanate from cathode tubes, causing fluorescence.

Answer 14

The Electron (Cathode Rays)

Question 15

J. J. Thomson is credited with their discovery (1897)

Answer 15

The Electron (Cathode Rays)

Question 16

Thomson measured the charge/mass ration of the electron to be 1.76x10 raise to the power of 8 coulombs/gram (C/g)

Answer 16

The Electrons

Question 17

Once the charge/mass ration of the electron was known, determination of either the charge or the mess of an electron would yield the other.

Answer 17

Millikan Oil-Drop Experiment (Electrons)

Question 18

Who determined the charge on the electron in 1909?

Answer 18

Robert Millikan

Question 19

It is the spontaneous emission of high-energy radiation by an atom.

Answer 19

Radioactivity

Question 20

It was fist observed by Henri Becquerel and Marie and Pierre Curie also studied it.

Answer 20

Radioactivity

Question 21

Its discovery showed that the atom had more subatomic particles and the energy associated with it.

Answer 21

Radioactivity

Question 22

The three types of radiation were discovered by Ernest Rutherford namely:

Answer 22

a particles (positively charged)
B particles (negatively charged, like electrons)
y rays (uncharged)

Question 23

The prevailing theory was that of the “plum pudding” model, put forward by Thomson. It featured a positive sphere of matter with negative electrons embedded in it.

Answer 23

The Atom, circa 1900

Question 24

Ernest Rutherford shot (a) particles at a thin sheet of gold foil and observed the pattern of scatter of the particles.

Answer 24

Discovery of the Nucleus

Question 25

Rutherford postulated a very small, dense nucleus with the electrons around the outside of the atom.

Answer 25

The nuclear atom

Question 26

The atoms of the same elements with different masses. It has different numbers of neutrons, but the same number of protons.

Answer 26

Isotopes

Question 27

It the average mass found using all isotopes of an element weighted by their relative abundances.

Answer 27

Atomic weight

Question 28

It is a systematic organization of the elements, and the elements are arranged in order of atomic number.

Answer 28

Periodic Table

Question 29

What are the rows on the periodic table called?

Answer 29

Periods

Question 30

What are the columns on the periodic table called?

Answer 30

Group

Question 31

This are composed of molecules and almost always contain only nonmetal.

Answer 31

Molecular compounds

Question 32

What are the seven elements that occur naturally as molecules containing two atoms?

Answer 32

Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine.

Question 33

It is the formula that gives the lowest whole-number ratio of atoms of each element in a compound.

Answer 33

Empirical formulas

Question 34

This formula gives the exact number of atoms of each element in a compound.

Answer 34

Molecular formulas

Question 35

This type of formula shows the order in which atoms are attached. They do not depict the three-dimensional shape of molecules.

Answer 35

Structural formulas

Question 36

It shows the three-dimensional order of the atoms in a compound. This are also demonstrated using models.

Answer 36

Perspective drawings

Question 37

When an atom of a group of atoms loses or gains electrons, it becomes?

Answer 37

Ion

Question 38

This are formed when at least one electron is lost.

Answer 38

Cations

Question 39

This are formed by metals.

Answer 39

Monatomic cations

Question 40

This are formed when at least one electron is gained.

Answer 40

Anions

Question 41

This are formed by nonmetals.

Answer 41

Monatomic anions

Question 42

This are generally formed between metals and nonmetals.

Answer 42

Ionic compounds