Chemistry Mini Test - Periodic Table
What are the only two liquid elements? Which one is a metal?
Bromine and Mercury; Mercury
Malleable
Capable of being changed; easily shaped
Conducts electricity
Metal
How many valence electrons in group 1
1
How many valence electrons in group 15
15
How many valence electrons in group 13
3
How many valence electrons in group 14
4
If an element's electron configuration ends in 3p2, in what row# and group# is it found?
4 and p
How many valence electrons in group 16
6
How many valence electrons in group 17
7
How many valence electrons in group 18
8
Conductor
A material that allows heat and electricity to pass through it.
Halogens
A nonmetal in Group 7A of the periodic table
What kind of important information is represented by the period numbers?
A period in the periodic table is a horizontal row. All elements in a row have the same number of electron shells. Each next element in a period has one more proton and is less metallic than its
Semiconductor
A substance that can conduct electricity under some conditions
Nonconductor
A substance that does not conduct heat or electricity
Periodic Table
A table that shows the elements, their atomic number, symbol, and average atomic mass; elements with similar chemical properties are grouped together, elements are arranged by their atomic mass
Ductile
A term used to describe a material that can be pulled out into a long wire
INCREASE electronegativity within a PERIOD
ACROSS - LEFT to RIGHT
Noble Gases
An element in group 8A of the periodic table; the s and p sublevels of the highest occupied energy level are filled (inert gases)
Inner Transition Metals
An element in the lanthanide of actinide series; the highest occupied s sublevel and nearby f sublevel of its atoms generally contain electrons; also called inner transition element
Negative Ions
Anions
Would highly elrctronegative atoms tend to form cations or anions?
Anions
Alkali Metals
Any metal in Group 1A of the periodic table
Alkali Earth Metals
Any metal in Group 2A of the periodic table
Explain WHY the trend for atomic radius within a period is the way it is.
Atomic radius decreases across a period because valence electrons are being added to the same energy level at the same time the nucleus is increasing in protons. The increase in nuclear charge attracts the electrons more strongly, pulling them closer to the nucleus.
Shielding electrons
Blocking electron appointment to a (+) nucleus
List all the metalloids:
Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Polonium, Astatine
Posative Ions
Cation
Explain WHY a cation is smaller than the atom it came from.
Cations are ALWAYS smaller than the atoms they came from (Na loses 1 e-, now more protons than e- so attraction is greater, pulls e- in close)
Nuclear charge
Charge of protons in the nucleus
Atomic Radii INCREASE withing a GROUP
DOWN - LEFT to RIGHT
INCREASE ionization energy within a GROUP
DOWN - RIGHT TO LEFT
Brittle
Easily broken; not flexible
Four periodic trends
Electron efficiency, atomic radii, ionized energy (IE), and electronegativity (EN)
Give the trend for valence electrons in the main group elements?
Elements in the same Group have the same number of valence shell electrons. Across a period of the Periodic Table from left to right the number of valence electrons increases.
Contrast nonmetals and metalloids.
Elements that have properties of both metals and nonmetals are called metalloids. They can be shiny or dull and their shape is easily changed. Electricity and heat can travel through metalloids but not as easily as they travel through metals.
Where on the periodic table would one expect to find elements that had similar properties ?
Elements within the same group have similar properties.
Where are the noble gases and why is their electronegativity 0?
Far right, they don't want filled electrons, they have filled octets
What element would have the highest electronegativity value? Why?
Flourine, its electrons are really close to the nucleus
What element would have the lowest EN?
Francium
INCREASE electronegativity within a GROUP
GO UP - INCREASE - LEFT to Right
Inert
Gases that do not form compounds
Where are the noble gases found?
Group 8A (18)
The vertical columns of the periodic table are also known as families or ____________________.
Groups
Where are the transition metals found?
Groups 3B - 2B (3 - 12)
Atomic radii
Half the distance between the nuclei of two atoms of the same element
Which elements are unreactive or inert? Why are they unreactive?
Helium(He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn) because their atoms have complete highest energy levels (full outer shells) of electrons
Main Group Elements
Helium, lithium, beryllium, boron,carbon, nitrogen, oxygen, and fluorine, groups 1A-8A (1,2,13-18)
Periods
Horizontal rows of elements in the periodic table
Contrast metals and metalloids.
In comparison with metals, metalloids are solid can be a conductor but in a fairly manner only. They also have higher densities compared to nonmetals and have a metallic appearance. In contrast, metalloids are more brittle compared with metals which are ductile and malleable if solid.
How does shielding change within a GROUP
Increases down
Describe the periodic trend for atomic size down a group and across a period.
Increases, atomic size increases down a group but decreases across a period
INCREASE ionization energy within a PERIOD
LEFT to RIGHT
Metal
Left of stair step line, one of a class of elements that are good conductors of heat and electric current, metals tend to be ductile, malleable, and shiny
Name an element that has properties similar to Na.
Lithium & Potassium
KNOW THE TRENDS and why.
Major periodic trends include: electronegativity,ionization energy, electron affinity, atomic radius, metallic character, ionic radius and reactivity. Periodic trends arise from the arrangement of elements in the periodic table and allow chemists to quickly and reliably predict an element's properties.
Ductile
Metal
Has luster
Metal
High boiling point
Metal
Malleable
Metal
In what 2 ways are metalloids similar to nonmetals?
Metalloids have properties of both metals and nonmetals. Metalloids can be shiny or dull. Electricity and heat can travel through metalloids, although not as easily as they can through metals. They are also called semimetals.
In what 2 ways are metalloids similar to metals?
Metalloids may act either like metals or nonmetals in chemical reactions.They fall between metals and nonmetals in their ability to conduct heat and electricity. They are shiny like metals but brittle like nonmetals. All exist as solids at room temperature.
How do metals, nonmetals, and metalloids compare with respect to location on the periodic table?
Metals: left to stair step line Nonmetals: to right of stair step line Metalloids: touching stair step line
Which is more electronegative? Ca or Mg? Cr or Ge? C or F?
Mg, Ge, F
Which is larger: O2- or Ne? Be or Mg? Na+ or Mg2+? Ba2+ or Xe?
Ne, Mg, Na+, Xe
Brittle, dull
Nonmetal
Nonconductor
Nonmetal
Reacts with acid
Nonmetal
Transition Metals
One of the Group B elements in which the highest occupied s sublevel and a nearby d sublevel generally contain electrons
What are the horizontal rows of the periodic table also called?
Periods
Name an element that has properties similar to N.
Phosphorus
Atomic Radii INCREASE within a PERIOD
RIGHT to LEFT
How does shielding change within a PERIOD
Remains constant
Non Metal
Right of stair step line, an element that tends to be a poor conductor of heat and electric current; nonmetals generally have properties opposite to those of metals
Describe where the following regions are on the periodic table: s, p, d, f.
S= left D=mid P=right F=bottom
What makes a metalloid like silicon a good material for computer chips?
Silicon is a metalloid, an element with properties of both metals and nonmetals.Silicon exists in two allotropic forms. Silicon is a semiconductor. A semiconductor is a substance that conducts an electric current better than a non-conductor—like glass or rubber—but not as well as a conductor—like copper or aluminum.
Most elements are which state of matter?
Solid
Which has a higher ionization energy? Sr or Mg? S or Cl? I or Br? WHY does each of these show that pattern?
Sr, Cl, I ; Increases left to right
Periodic Law
States that when the elements are arranged by increasing atomic number, there is a periodic repetition of their properties
What is electronegativity?
The ability of an atom of an element in a compound to attract electrons
The metals are separated from the nonmetals on the periodic table by the __________________.
The diagonal line at the right side of the table
Electron affinity
The energy released when adding an electron to an atom
What is electronegativity?
The energy required to remove an electron from a gaseous atom
What causes ionization energy to increase going across a period?
The general trend is for ionisation energies to increase across a period. That causes greater attraction between the nucleus and the electrons and so increases the ionisation energies. In fact the increasing nuclear charge also drags the outer electrons in closer to the nucleus.
What is ionization energy?
The minimum amount of energy required to remove an electron from a gaseous atom
What causes ionization energy to decrease going down a group?
The number of electrons increases and the strength of shielding increases. As a result, it is easier for valence shell electrons to ionize, and thus the ionization energy decreases down a group. Electron shielding is also known as screening. This is due to electron shielding.
Explain WHY atomic radius increases down within a group.
The number of energy levels increases as you move down a group as the number of electrons increases. Each subsequent energy level is further from the nucleus than the last. Therefore, the atomic radius increases as the group and energy levels increase.
Where are the metalloids found?
Touching stair step line
Metalloid
Touching stair step, an element that tends to have properties of both metals and nonmetal
Where on the periodic table would you find most of the gases?
Upper right corner
Groups or Families
Vertical columns
What does it mean to describe something as periodic?
You describe something as periodic, because something periodic can happen only after a period of time