Chem Ch 5 Test Flashcards
What is the difference between periods and groups/families on the periodic table?
Period- left to right. Same number of electron orbitals
Groups- Up down. Same number of valence electrons
Who organized elements in groups of threes and fours based on similar properties?
Dobreiner
Newlands used what to organize the elements? Were his ideas accepted?
Atomic mass. No
What form of energy did Henry Moseley use to determine the atomic numbers of elements?
Frequency of x-ray
Which one of these is not an element symbol? O H HN Cu
HN
Transition metals occupy which numbered groups on the periodic chart?
Groups 3-12
Alkali metals occupy which numbered group on the periodic chart?
Group 1
Alkaline earth metals occupy which numbered group on the periodic chart?
Group 2
Noble gases occupy which numbered group on the periodic chart?
Group 18
Halogens occupy which numbered group on the periodic chart?
Group 17
Which side of the table do you find metals on left, right center or bottom?
Left and middle
Which side of the table do you find nonmetals on left, right center or bottom?
Right
Francium is in the lower left section of the periodic table, and Fluorine is in the upper right. Which has the larger atomic radius?
Francium
How does the size of a metal atom compare to its positive ion? Its negative ion?*
Positive (Cation)- Bigger
Negative (Anion)- Smaller
Ionization energy
Measures the energy required to remove an outermost electron
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?
Radium
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
Electron affinity
Property that measures the attraction of bonded atoms to electrons
Electronegativity
A sample of an unidentified element has a bright luster, conducts electricity well, and is highly reactive. It is most likely what
Alkali metals
Semiconductors can also be called __________. What do they do?
Metalloids. Conduct electricity but only under certain conditions
The halogens form __________ when they combine with metals and __________ when they combine with hydrogen
Salts/acids
What are examples of Halogens?.
Fluorine, Chlorine, Bromine, Iodine, Astatine,
Who left blanks on his periodic table?
Mendeleev
Atomic radii does it increase or decrease as you go from left to right on the periodic table?
Why?
Decreases because more protons means more attraction for electrons. Results in shrinking of atomic radius
Atomic radii does it increase or decrease as you go from top to bottom on the periodic table?
Why?
Increases because going down a group or family add extra layer of electrons for each level
Explain what is the trend in ionization energy going down a group and across a period. Also, explain why these trends are there.
Down decrease, further from nucleus easier to remove
Right increase, closer to nucleus, more protons = more attraction, harder to remove
Electron affinity
Amnt of energy required to add electron to neutral atom to form negative ion
Opposite of ionization energy
Electronegativity
Measure of attraction btwn nucleus and valence electrons
Determined for atoms bonded in molecules
Alkaline Earth metals
Group 2
Denser, harder, higher melting points than alkali metals
Typically donate 2 electrons
Ex: Military flares, x-rays, bones
Transition metals
Shinier, harder, denser than groups 1&2
Some react easily some don’t
Ex: coin, jewelry, wire
Inner transition metals
Paramagnetism- weak attraction to magnetic field
Actinide series- highly radioactive
Used in glass and atomic bombs
Post transition metals
Groups 13-16
Metalloids- characteristics lying between those of metals and nonmetals
Semiconductors- conduct electricity under certain conditions
Boron family
Group 13
Boron- conducts electricity at high temps
Aluminium- shiny, low density
Carbon family
Group 14
Nonmetal; no reactive at room temp
Bond with anything
4 valence electrons
Oxygen family
Group 16
Exists as O2 and O3
Nonmetal- fairly nonreactive at room temp
Colorless, odorless, tasteless
Oxides and sulfites
Sulfur- reactive at room temp
Halogen family
Group 17
More color, higher melting point, density
Most reactive out of all nonmetals
Used for halogen lights, bleach and medical uses
Noble gas family
Group 18
Colorless, odorless, tasteless
Rarely react
Used for balloons, diving, neon light
Nitrogen family
Normally diatomic gas
Colorless, odorless, tasteless
Phosphorus rarely found itself in nature
Inert (doesn’t react)
