Chemistry Ch 6 Practice
Identify the representative elements from the list given below. Na, Ca, Sc, Co, Ni, Si, N, Se, Cl, Ge
Na, Ca Si, N, Se, Cl, Ge
Why is the argon placed before potassium in the modern periodic table.?
Smaller atomic number
Which block contains 5 orbitals? A. s B. p C. d D. f
A
Which block on the periodic table contains the actinide series of elements? A. s-block B. p-block C. d-block D. f-block
D
Which is the transition element with five d-block electrons in energy level 4? A. Niobium (Nb) B. Renium (Re) C. Manganese (Mn) D. Technicium (Tc)
D
Which property describes how much energy must be added to an atom to remove an outermost electron? A. atomic radius B. ionic radius C. electronegativity D. ionization energy
D
Which region is referred to as the p-block on the diagram? A, B, C, D
D
Which scientist first arranged elements by atomic number? A. Mendeleev B. Lavoisier C. Newlands D. Mosely
D
T/F: All of the nonmetals on the periodic table are gases.
False
Which element is the most metallic? A, B, C, D
A
Which block is element Y most likely found? A. s B. p C. d D. f
B
Which category of elements have the property f being malleable and ductile? A. Gases B. Metals C. Metalloids D. Nonmetals
B
Which category of elements in commonly used to make computer chips and solar cells due to their ability to conduct electricity only under certain conditions? A. Metals B. Metalloids C. Nonmetals D. Noble Gases
B
Which diagram correctly depicts the general trend in first ionization energy? A, B, C, D
B
Which diagram correctly depicts the trend in electronegativity? A, B, C, D
B
Which region contains the alkaline earth metal family of elements? A, B, C, D
B
T/F: An atom that gains an electron will form a positive ion.
False
Define ionization energy.
the closer the electrons are to the nucleus of the atom, the higher the atom's ionization energy
Label the blank periodic table with the following terms. A. metalloids B. element with the highest electronegativity C. alkali metals D. lanthanide series E. element with the greatest atomic radius F. noble gases G. halogens
..
According to _________ period table, the physical and chemical properties of elements are periodic functions of their atomic weights. A. Dmitri Mendeleev's D. John Newlands' C. Henry Mosely's D. Lothar Meyer's
A
Which correctly describes elements in the same group? A. They have the same number of valence electrons. B. The have electrons in the same outermost energy level. C. They have the same atomic radius. D. They must be in the same state of matter.
A
Which is defined as the energy required to remove an electron from an atom of an element in the gaseous state? A. ionization energy B. electronegativity C. ionin radius D. loaw of octets
A
Which region contains elements with two valence electrons?A, B, C, D
A
Two elements A and B have atomic numbers 8 and 17 respectively. Identify their groups in the periodic table.
A: 6A B: 7A
Which element has an electron configuration that ends in the fourth energy level? A, B, C, D
B
Which is the energy level that is being filled by electrons in the transition elements of period 5? A. third B. fourth C. fifth D. sixth
B
Which metalloid is in the fourth period and the same group as Carbon? A. Silicon B. Germanium C. Tin D. Boron
B
Which region is referred to as the f-block on the diagram? A, B, C, D
B
Which scientist classified elements into four categories: gases, metals, nonmetals, & metalloids? A. Mendeleev B. Lavoisier C. Newlands D. Mosely
B
Arrange the elements given below in the increasing order of their atomic size. A. 1s^2 2s^2 2p^6 B. 1s^2 2s^2 C. 1s^2 2s^2 2p^6 3s^1 D. 1s^2 2s^2 2p^3
B, A, D, C
Place these five elements in order of electronegativity, with the high electronegativity first.
B, D, C, E, A
Identify the period and group numbers of the element with the electron configuration. [Ne} 3s^2 3p^4 A. Period 2, Group 4 B. Period 3, Group 4 C. Period 3, Group 16 D. Period 2, Group 16
C
Which group will have an electron configuration that ends in "n"s^2? A. Alkali metals B. Alkaline Earht Metals C. Halogens D. Actinides
C
Which is the most important characteristic in determining an element's chemical properties? A. the number of protons and neutrons in its nucleus B. which period it is found in C. the number of valence electrons it contains D. its outermost energy level
C
Which of the following elements is a metal? A. Boron B. Nitrogen C. Magnesium D. Carbon
C
Which region contains elements with an electron configuration that ends with p^3? A, B, C, D
C
Which region contains the halogen family of elements? A, B, C, D
C
Which scientist characterized the "law of octaves"? A. Mendeleev B. Lavoisier C. Newlands D. Mosely
C
hich is the halogen that is in Period 5? A. Bromine (Br) B. Strontium (Sr) C. Iodine (I) D. Xenon (Xe)
C
Write the electron dot structure of the element of 7A group and third period.
Cl with 7 dots
In which pair is the one on the left larger than the one on the right? A. Na, Rb B. S, Mg C. Br, Br- D. K, K+
D
T/F: Although chemical properties obey the periodic law, it is impossible to predict physical properties of elements based on their location in the periodic table.
False
T/F: Elements in group 2 are classified as alkali metals.
False
T/F: The electronegativity of elements increases from left to right and from top to bottom on the periodic table.
False
T/F: The same amount of energy is required to remove each electron sequentially from an atom.
False
T/F: The transition elements consist only of those that are found in block d of the period table.
False
Explain what is meant by the "law of octaves." Does it hold true for the modern period table?
If the chemical elements are arranged according to increasing atomic weight, those with similar physical and chemical properties occur after each interval of seven elements. The pattern is set up into eighths, so it does not hold true.
Use the periodic table to write the names of the third alkali metal and the first transition metal.
K, Scandium
A student makes the following statement: "It's easy to tell which energy level an element is in - you just count down which row it is in, and that;s the energy level." Is this student correct? Explain how you came to your conclusions.
No. Periods are not the same as the electron configurations that are given.
Why do elements in the same group have similar properties?
Number of valence electrons are the same
The second ionization energy of sodium is very high as compared the to the first ionization energy. Explain this trend in sodium.
Related to the number of valence electrons, sodium is not likely to hold a 2+ sodium, it would take too much energy to produce a new electron
Do the figures in this periodic table demonstrate the trend in atomic radius, ionic radius, or neither of these? Relate your answer to the structure of atoms across the periodic table.
Show atomic radius change, moving across & gaining electrons pull the nucleus tighter making the size of the atom decrease
What are phosphors? Give examples from the periodic table.
Substances that emit light, lanthanide series
An element has similar chemical properties as oxygen and selenium. It has an atomic number greater than krypton but less than iodine. Use the periodic table to identify the element.
Tellurium
State the periodic law.
The law that the properties of the elements are periodic functions of their atomic numbers.
Explain the significance of the stair-step line located near the right-hand side of the periodic table.
The stair-step line separates metal from nonmetals& designates metalloids.
T/F: Elements in group 17 are classified as halogens.
True
T/F: Elements in the same family tend to have the same number of valence electrons.
True
T/F: The octet rule states that atoms will gain, lose, or share electrons to achieve a complete set of eight valence electrons.
True
T/F: The radius of an atom is defined as half the distance between the nuclei of two adjacent or bonded atoms of that element.
True
T/F: When an atom loses electrons, it radius gets smaller.
True
Identify the element having the largest size and the element have the highest electronegativity from the list of electron configurations given below: a. [Ne] 3s^23p^3 b. [Ne]3s^23p^4 c. [Ne] 3s^2 3p^5 d. [Ne] 3s^2 3p^6 4s^2 3d^3
a. highest electronegativity d. largest size
The group 2A elements are known as _____________.
alkaline earth metals
Elements that have physical and chemical properties of both metals and nonmetals are known as ____________.
metalloids
Why is the size of a sodium ion (Na+) less than that of a sodium atom (Na)?
results in a smaller radius by loosing an electron pulling in the protons
List the general electron configuration and location of the s, p, d, and f-block elements in the periodic table.
s: 1-2 p: 13-18 d:3-12 f: lanthanide & actinide
Predict the position of an element with electron configuration (n-1)d^1, (n)s^2, where n=4
scandium
