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CDA- 17 Study Guide
Periodicity of the Elements
40
Science
8th Grade
02/20/2010

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Term
______ proposed that the properties of the elements vary in a periodic manner with the atomic weight of the elements.
Definition
Dmitri Mendeleev
Term
Mendeleev grouped elements with similar properties in __rows __columns __groups of eight
Definition
columns
Term
In 1914 _____ found that the frequency of vibration of the X-rays emitted by each element when bombarded with cathode rays bore a simple relationship to the atomic numbers
Definition
Henry Mosely
Term
Complete the following: The periodic law specifies...
Definition
"... the chemical properties of the elements are periodic functions of their atomic numbers."
Term
What determines the "energy level" of an electron?
Definition
The distance of the electron from the proton-containing nucleus.
Term
T/F~ The MORE energetic electrons orbit closest to the nucleus.
Definition
false
Term
Who developed the "planetary model" of the atom?
Definition
Niles Bohr
Term
T/F~ SEVEN is the maximal number of electron layers that any atom can contain.
Definition
true
Term
T/F~ Each of the energy levels has a limit on the number of electrons it can hold.
Definition
true
Term
How many electrons can the third energy level hold?
Definition
18
Term
What equation specifies the maximum number of electrons an energy level can hold?
Definition
2n 2(exponent!)
Term
What is the "octet rule"?
Definition
"The maximum number of electrons in the outermost energy level is 8"
Term
What is the "electron configuration?"
Definition
"The number and position of electrons in the energy levels of an atom."
Term
What is the electron configuration of the atom with an atomic number equal to 8?
Definition
level 1 = 2, level 2 = 6
Term
What is the electron configuration of the atom with an atomic number equal to 16?
Definition
level 1 = 2, level 2 = 8, level 3 = 6
Term
What is the electron configuration of the atom with an atomic number equal to 20?
Definition
level 1 = 2, level 2 = 8, level 3 = 8, level 4 = 2
Term
The electrons in the outermost energy level are called...
Definition
valence electrons
Term
What about the valence electrons is so important to the field of chemistry?
Definition
The ability of the atom to gain or lose the valence electrons is what determines it's chemical properties. Most chemical reactions involve the valence electrons; electrons in the inner layers are not important in normal circumstances.
Term
Elements in the periodic table are arranged in what two ways?
Definition
Horizontally in rows in the order of increasing atomic number; vertically in columns according to their chemical properties.
Term
T/F~ All elements in vertical columns have same number of valence electrons.
Definition
true
Term
T/F~ Rows in the periodic table are called families or groups.
Definition
false
Term
The alkali metals are located in what group number?
Definition
1 or 1A
Term
The halogens are located in what group number?
Definition
17 or VIIA
Term
The noble gases are located in what group number?
Definition
18 or VIIIA
Term
The alkaline earth metals are located in what group number?
Definition
2 or IIA
Term
T/F~ Chemical properties change across rows, that is as you move from left to right within a period.
Definition
true
Term
T/F~ With reference to the electronic configuration a new layer is added for each row or period in the periodic table.
Definition
true
Term
T/F~ The energy lovel of the valence electrons is determined by the period it is in.
Definition
true
Term
T/F~ The shape of the periodic table tells us where all of the electrons are in an atom.
Definition
true
Term
T/F~ The maximal number of electrons in energy level 7 is 98
Definition
true
Term
Locate aluminum in the periodic table. How many valence electrons is there in a neutral atom of aluminum?
Definition
3
Term
What is the dominant chemical property of the alkali metals group?
Definition
They easily lose theri single valence electron. Thurs they are highly chemically reactive, especially with non mentals.
Term
What are the two most common valences for the "transition elements?"
Definition
1 and 2
Term
T/F~ The alkali metals exist in nature as diatomic molecules.
Definition
false
Term
Why are the halogens so extremely reactive chemically?
Definition
They seek an electron to complete their outermost electron level. We say they are highly electronegative.
Term
List the three classes of elements and designate their relative positions in the periodic table.
Definition
metals are on the left side; nonmetals are on the extreme right side; metalloids are in between.
Term
List four properties of metals.
Definition
Conductors of heat and electricity; will lose electrons when reacting with nonmetals; lustrous, malleable, and ductile; have high tensile strength; all are solids at room temperature except for mercury.
Term
Most metals are hard, strong and dense. Provide two examples of metals that are the exceptions to this.
Definition
Sodium (Na) is soft- you can cut it with a knife; Mercury (Hg) is a liquid. Maganese (Mn) is brittle.
Term
T/F~ Metals belong to the families of elements with few electrons (1,2,or3) in the outer energy level.
Definition
true
Term
T/F~ Metals do not hold their valence electrons strongly and give them up easily.
Definition
true
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