Chem Ch 5 Test

Question 1

What is the difference between periods and groups/families on the periodic table?

Answer 1

Period- left to right. Same number of electron orbitals
Groups- Up down. Same number of valence electrons

Question 2

Who organized elements in groups of threes and fours based on similar properties?

Answer 2

Dobreiner

Question 3

Newlands used what to organize the elements? Were his ideas accepted?

Answer 3

Atomic mass. No

Question 4

What form of energy did Henry Moseley use to determine the atomic numbers of elements?

Answer 4

Frequency of x-ray

Question 5

Which one of these is not an element symbol? O H HN Cu

Answer 5

HN

Question 6

Transition metals occupy which numbered groups on the periodic chart?

Answer 6

Groups 3-12

Question 7

Alkali metals occupy which numbered group on the periodic chart?

Answer 7

Group 1

Question 8

Alkaline earth metals occupy which numbered group on the periodic chart?

Answer 8

Group 2

Question 9

Noble gases occupy which numbered group on the periodic chart?

Answer 9

Group 18

Question 10

Halogens occupy which numbered group on the periodic chart?

Answer 10

Group 17

Question 11

Which side of the table do you find metals on left, right center or bottom?

Answer 11

Left and middle

Question 12

Which side of the table do you find nonmetals on left, right center or bottom?

Answer 12

Right

Question 13

Francium is in the lower left section of the periodic table, and Fluorine is in the upper right. Which has the larger atomic radius?

Answer 13

Francium

Question 14

How does the size of a metal atom compare to its positive ion? Its negative ion?*

Answer 14

Positive (Cation)- Bigger
Negative (Anion)- Smaller

Question 15

Ionization energy

Answer 15

Measures the energy required to remove an outermost electron

Question 16

Magnesium is in Group 2 (2A) and Period 3 of the periodic table, and radium is in Group 2 (2A) and Period 7. Which has the smaller ionization energy?

Answer 16

Radium

Question 17

Which property measures the energy released when an electron joins an atom?
a. atomic size
b. ionic size
c. ionization energy
d. electron affinity
e. electronegativity

Answer 17

Electron affinity

Question 18

Property that measures the attraction of bonded atoms to electrons

Answer 18

Electronegativity

Question 19

A sample of an unidentified element has a bright luster, conducts electricity well, and is highly reactive. It is most likely what

Answer 19

Alkali metals

Question 20

Semiconductors can also be called __________. What do they do?

Answer 20

Metalloids. Conduct electricity but only under certain conditions

Question 21

The halogens form __________ when they combine with metals and __________ when they combine with hydrogen

Answer 21

Salts/acids

Question 22

What are examples of Halogens?.

Answer 22

Fluorine, Chlorine, Bromine, Iodine, Astatine,

Question 23

Who left blanks on his periodic table?

Answer 23

Mendeleev

Question 24

Atomic radii does it increase or decrease as you go from left to right on the periodic table?
Why?

Answer 24

Decreases because more protons means more attraction for electrons. Results in shrinking of atomic radius

Question 25

Atomic radii does it increase or decrease as you go from top to bottom on the periodic table? Why?

Answer 25

Increases because going down a group or family add extra layer of electrons for each level

Question 26

Explain what is the trend in ionization energy going down a group and across a period. Also, explain why these trends are there.

Answer 26

Down decrease, further from nucleus easier to remove Right increase, closer to nucleus, more protons = more attraction, harder to remove

Question 27

Electron affinity

Answer 27

Amnt of energy required to add electron to neutral atom to form negative ion Opposite of ionization energy

Question 28

Electronegativity

Answer 28

Measure of attraction btwn nucleus and valence electrons Determined for atoms bonded in molecules

Question 29

Alkaline Earth metals

Answer 29

Group 2 Denser, harder, higher melting points than alkali metals Typically donate 2 electrons Ex: Military flares, x-rays, bones

Question 30

Transition metals

Answer 30

Shinier, harder, denser than groups 1&2 Some react easily some don’t Ex: coin, jewelry, wire

Question 31

Inner transition metals

Answer 31

Paramagnetism- weak attraction to magnetic field Actinide series- highly radioactive Used in glass and atomic bombs

Question 32

Post transition metals

Answer 32

Groups 13-16 Metalloids- characteristics lying between those of metals and nonmetals Semiconductors- conduct electricity under certain conditions

Question 33

Boron family

Answer 33

Group 13 Boron- conducts electricity at high temps Aluminium- shiny, low density

Question 34

Carbon family

Answer 34

Group 14 Nonmetal; no reactive at room temp Bond with anything 4 valence electrons

Question 35

Oxygen family

Answer 35

Group 16 Exists as O2 and O3 Nonmetal- fairly nonreactive at room temp Colorless, odorless, tasteless Oxides and sulfites Sulfur- reactive at room temp

Question 36

Halogen family

Answer 36

Group 17 More color, higher melting point, density Most reactive out of all nonmetals Used for halogen lights, bleach and medical uses

Question 37

Noble gas family

Answer 37

Group 18 Colorless, odorless, tasteless Rarely react Used for balloons, diving, neon light

Question 38

Nitrogen family

Answer 38

Normally diatomic gas Colorless, odorless, tasteless Phosphorus rarely found itself in nature Inert (doesn’t react)