Chapter 6

Question 1

Antoine Lavoisier

Answer 1

Compiled a list of 23 known elements.

Question 2

John Newlands

Answer 2

Noticed that when elements are arranged by increasing atomic mass, their properties repeated every 8 elements. The law of octaves. It was not accepted because it did not work for all known elements. People thought the musical analogy was unscientific so they rejected it.

Question 3

Lothar Meyer

Answer 3

Demonstrated a connection between atomic mass and elemental properties in the same year as Mendeleev, but is given less credit because he published his organization scheme later, and Mendeleev predicted properties about elements yet to be discovered.

Question 4

Dmitri Mendeleev

Answer 4

Noticed that when elements are arranged by increasing atomic mass, there was a periodic pattern in their properties. By arranging the elements in order of increasing atomic mass into columns with similar properties, Mendeleev organized the elements into the first periodic table.

Question 5

Which elements’ properties was Mendeleev able to predict?

Answer 5

Scandium, Gallium, Germanium

Question 6

Henry Moseley

Answer 6

Solved the problems with Mendeleev’s table by arranging the elements by atomic number.

Question 7

Periodic Law

Answer 7

There is a periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number.

Question 8

(T/F) Groups/Families are Horizontal

Answer 8

Vertical

Question 9

(T/F) Periods are Horizontal

Answer 9

True

Question 10

Representative Elements

Answer 10

Groups 1-2 and 13-18. Their last filled electron is a valence electron. They have a wide range of chemical and physical properties

Question 11

Transition Elements

Answer 11

Groups 3-12, which have electrons that have just been filled in the D or F orbitals.

Question 12

What are the 3 main classifications for the elements?

Answer 12

Metals, nonmetals, metalloids/semi-metals

Question 13

Metals

Answer 13

Elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors of heat and electricity.

Question 14

(T/F) Metals are malleable but not ductile

Answer 14

Metals are malleable (Can be pounded into thin sheets) AND ductile (Can be stretched into wires)

Question 15

(T/F) All group B elements are metal

Answer 15

True

Question 16

What is the one element on the left side of the periodic table that is not a metal?

Answer 16

Hydrogen

Question 17

1A/1 (Except for H)

Answer 17

Alkali metals

Question 18

2A/2

Answer 18

Alkaline Earth metals

Question 19

What are the two sets of inner transition metals?

Answer 19

The lanthanide and the actinide series

Question 20

Does the Lanthanide series come first or the Actinide series?

Answer 20

The Lanthanide series comes first. It is in period 6 while the Actinides are in period 7.

Question 21

Transition metals

Answer 21

Elements in groups 3-12.

Question 22

(T/F) Elements from the actinide series are used to make phosphors

Answer 22

Elements from the LANTHINIDE series are used to make phosphors (substances that emit light when struck by electrons)

Question 23

What is in the upper right hand corner of the periodic table?

Answer 23

Nonmetals

Question 24

Nonmetalls are elements that…

Answer 24

Are generally gasses or brittle, dull looking solids. They are poor conductors of heat and electricity.

Question 25

(T/F) There are no liquid nonmetals at room temperature

Answer 25

Bromine is the only nonmetal that is a liquid at room temperature.

Question 26

7A/17

Answer 26

Halogens (Highly reactive)

Question 27

8A/18

Answer 27

Noble gasses

Question 28

Metalloids

Answer 28

Elements with physical and chemical properties of both metals and nonmetals.

Question 29

What two metalloids are used in computer chips and solar cells?

Answer 29

Silicon and Germanium

Question 30

Atoms in the same group have the same properties because ____

Answer 30

They have the same number of valence electrons. For example, in group 1A, all the valence shells have a configuration of _s1

Question 31

The outermost energy level that an atom has electrons in is also the same as the atom’s ______ on the periodic table

Answer 31

Period

Question 32

S Block elements

Answer 32

Groups 1 and 2, the alkali metals and the alkaline earth metals. Characterized by full or partially filled S orbitals.

Question 33

P block elements

Answer 33

Groups 13-18 with valence electrons in the P orbital. Characterized by full or partially filled P orbitals.

Question 34

D block elements

Answer 34

Contains the transition metals; is the largest of the blocks. Characterized by full or partially filled D orbitals.

Question 35

F block elements

Answer 35

Contains the inner transition metals. Characterized by full or partially filled F orbitals.

Question 36

Atomic Radius

Answer 36

Half the distance between adjacent nuclei of a crystal of an element, or half the distance between nuclei of identical atoms that are chemically bonded to each other.

Question 37

The atomic radius increases as you go _____ and _____

Answer 37

Down and left.

Question 38

Explain the atomic radius period trend.

Answer 38

As you go across a period, there are more protons, but they are all on the same energy level. Therefore, since the atomic charge is greater, the atomic radii get smaller. Valence electrons, because the principal energy level is the same, do not get increased shielding from the positive charge.

Question 39

Explain the atomic radius group trend.

Answer 39

The atomic radii increase as you go down a group because as you go down a group, there are more energy levels. Therefore, the atomic radius gets bigger. The nuclear charge pull is overpowered because there is increased shielding from the positive charge.

Question 40

Ion

Answer 40

An atom or bonded group of atoms that has a positive or negative charge

Question 41

Ionic radius period trend

Answer 41

As you go across a period, the representative elements on the left side form increasingly small ions. Then, beginning in group 5A, the size of much larger negative ions gradually decreases.

Question 42

Explain the Ionic radius period trend

Answer 42

Atoms on the left side of the periodic table lose electrons, so they become smaller. Atoms on the right side gain electrons so they become bigger.

Question 43

Ionic radius group trend

Answer 43

As you go down a group, the atoms get bigger, so the ionic radii get bigger as well.

Question 44

Ionization energy

Answer 44

The energy required to move an electron from a gaseous atom.

Question 45

Ionization energy trends

Answer 45

As you go across a period, it gets bigger. However, there are some exceptions. An atom would rather have sets of full orbitals, so occasionally, the period trend will be broken. As you go down a group, the IE gets smaller because the electrons are further away from the nucleus.

Question 46

Octet rule

Answer 46

Atoms tend to gain, lose, or share electrons in order to acquire a full set of eight valence electrons.

Question 47

Electronegativity

Answer 47

The ability of an element to attract electrons in a chemical bond

Question 48

Electronegativity trend

Answer 48

As you go from left to right, there is increasing electronegativity. As you go from top to bottom there is decreasing electronegativity. F is the most electronegative element.

Question 49

Diagonal relationships

Answer 49

Some elements in period 2 do not behave as predicted by their locations on the table. Often, these elements have more in common with the period 3 element in the next group.