Chem 112 (Review) - Chp 6 Flashcards
What is another name for the representative elements?
Group A/main group elements
What is another name for the transition metals?
D Block Elements
Which elements are in the same period as phosphorus?
Na, Mg, Al, Si, P, S, Cl, and Ar
The modern period table is arranged in order of atomic “ “
Number
Who arranged the elements according to atomic mass and use the arrangement to predict the properties of missing elements?
Dmitri Mendeleev
Which general category of elements includes the majority of elements?
Metals
Of the elements Pt, V, Li, and Kr which are a nonmetal?
Kr is a nonmetal element.
To what category of elements does an element belong if it is poor conductor of electricity?
Nonmetals
In which of the following sets is the symbol of the elements, the number of protons, and the number of electrons given correctly?
(a) In - 49 protons and 49 electrons
(b) Zn - 30 protons and 60 electrons
(c) Cs - 55 protons and 132.9 electrons
(d) F - 19 protons and 19 electrons
*ANSWER: A*
The atomic number of an element is the total number of which particle in the nucleus?
Protons
What element has the electron configuration of 1s2, 2s2, 2p6, 3s2, 3p2?
Silicon (Si)
What is true about electron configurations of all noble gases?
The highest occupied sublevels “s” and “p” are completely filled
Where can you find the representative elements on the periodic table?
1 & 2 and 13-18
How does atomic radius change from top to bottom in a group in the periodic table?
Going down, it will increase.
How does atomic radius change from left to right across a period in the periodic table?
Decreases from left to right.
What causes the shielding effect to remain constant across a period?
The number of energy levels are the same.
What element in the second period has the largest atomic radius?
Lithium (Li)
What is the charge of a cation?
A positive charge
How are cations formed?
When an atom/compound loses, one or more electrons.
How are anions formed?
When an atom gains one or more electrons.
What are the charges of ions formed from the following elements? Na, Mg, Al, N, O.
Na: 1
Mg: 2
Al: 13
N: 15
O: 16
What is the element with the lowest electronegativity value?
Francium
What is the element with the highest electronegativity value?
Fluorine
What is the energy required to remove an electron from an atom in the gaseous state called?
Ionization energy
Which of the following elements has the smallest first ionization energy?
(a) sodium
(b) calcium
(c) potassium
(d) magnesium
ANSWER: C
Which of the following elements has the lowest electronegativity?
(a) lithium
(b) carbon
(c) bromine
(d) fluorine
ANSWER: A
Which statement is true about electronegativity?
(a) electronegativity is ability of an anion to attract another anion.
(b) electronegativity generally increases as you move top to bottom with a group.
(c) electronegativity generally is higher for metals than for nonmetals.
(d) electronegativity generally increases from left to right across a period.
ANSWER: D
Which of the following decreases with increasing atomic number and group 2A?
(a) shielding effect
(b) ionic size
(c) ionization energy
(d) number of electrons
What happens to the relative size of an atom when it becomes a cation?
becomes SMALLER than the atom
What happens to the relative size of an atom when it becomes a anion?
becomes a LARGER atom
Which group of elements in the periodic table is known as the alkali metals?
Group 1A
Which group in the periodic table is known as noble gases?
Group 18
An element has atomic number of 80. How many protons and electrons are in an atom of the elements?
80 protons and 80 electrons (equal)
What is the electron configuration of oxygen?
1s2 , 2s2 , 2p4 : Oxygen
What is the electron configuration of sulfur?
[Ne] 3s2 and 3p4 : Sulfur
The “S” and “P” sublevels of an atom of an element in period three are filled with electrons. Which orbitals are filled in this atom?
3s and 3p
What orbital is filled with iodine gains an electron to become a negative ion?
5p orbital
How many electrons are present in the D sub level of a neutral atom of nickel?
8 electrons in the “D” orbital
How many electrons are in rubidium ion (Rb+)?
37 electrons
What is the usual charge on an ion from group 7A?
Charges “-1”
How many electrons does the ion Ca2+ contain?
18 electrons
(20-2=18)
Explain how ions form. Provide examples.
When an atom gains/loses electrons in order to find a more stable configuration.
-> chlorine takes an electron from sodium, then sodium gives the electron chlorine that creates “NaCl”
What is electronegativity? Describe the trends in electronegativity within groups and across periods in the periodic table. Provide examples.
The ability of an atom to attract electrons when the atom is in a compound.
-> INCREASES when moving left to right and DECREASES as you move down in a group.
How do they measure atomic radius? Why does the atomic radius decrease as you move across the periodic table?
Atomic radius is measured in picometers (1x10^-12)
-> valence electrons are being added to the same energy level at the same time. The nucleus is INCREASING in protons.
What does ionization energy mean? For the elements in group 2A, compare the relative values of their first, second and third ionization energy and explain why this is.
Energy that is required to remove an electron from an atom in its gaseous state.
-> first - low
-> second - high
-> third - highest
