Chemistry Periodic Table Quiz
In the current periodic table, elements are arranged according to
atomic number
As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally
decreases
alkaline earth metals are
denser and stronger than alkali metals
Endothermic
energy is absorbed as a reactant A + e- + energy ➡️ A-
The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as
first ionization energy
Anions (-)
gained electrons Larger bc they are gaining electrons *The smaller the atom the much harder it is to lose an ion*
Properties of metals
good conductors of heat and electricity Malleable (easy to mold) Ductile High tensile strength Luster
atomic radius
half the distance between two nuclei of a diatomic molecule Why larger going down? -Higher energy levels have larger orbitals -Shielding-core: e- block the attraction between the nucleus and the valence e- Why smaller to the right? -Increased nuclear charge w/o additional shielding pulls e- in tighter
properties of metalloids
have properties of both metals and nonmetals B, Si, Ge, As, Sb, Te, Po
Which properties are most common in nonmetals?
high ionization energy and high electronegativity
As each successive element in Group 15 of the Periodic Table is considered in order of increasing atomic number, the atomic radius
increases
What is the total number of valence electrons in an atom of boron in the ground state?
3
What is the total number of valence electrons in an atom of xenon, Xe?
8
Electronegativity
A measure of the ability of an atom in a chemical compound to attract electrons
Which sequence of elements is arranged in order of decreasing atomic radii?
A) Al, Si, P B) Li, Na, K C) Cl, Br, I D) N, C, B A
Which list of elements from Group 2 on the Periodic Table is arranged in order of increasing atomic radius?
A) Be, Mg, Ca B) Ca, Mg, Be C) Ba, Ra, Sr D) Sr, Ra, Ba A
Which of the following atoms has the largest atomic radius?
A) Na B) K C) Mg D) Ca B
Which element in Period 5 of the Periodic Table is a transition metal?
A) Sr B) Sb C) Ag D) Xe Ag
Which statement is true?
A) the modern periodic table was developed at the First Congress of Chemists B) Motion needs to vary uniformly in order to vary periodically C) in his periodic table, Mendeleev arranges the Elemis in order of their atomic numbers D) Mendeleev left "gaps" in his periodic table to account for missing elements (D)
Which statement is true of alkali metals?
A) they are usually stored in water B) they are found in nature as free elements C) they are unable to combine with nonmetal elements D) they are soft enough to cut with a knife (D)
Which ion has a larger radius? Al or Al+3
Al
Which atom has a larger radius? Be or Ba?
Ba
Which of the following Group 2 elements has the lowest first ionization energy?
Ba
diamotic elements
Br2 I2 N2 Cl2 H2 O2 F2
Exothermic
Chemical Reaction in which energy is primarily given off in the form of heat A + e- ➡️ A- + energy
As the elements of Group 1 of the Periodic Table are considered in ordered from top to bottom, the ionization energy of each successive element decreases. This decrease is due to?
Decreasing radius and increasing shielding effect
Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?
Dmitri Mendeleev
The strength of atom's attraction for the electrons in a chemical bond is the atom's
Electronegativity
True or False: elements in the d-block are know as representative elements
False
True or false: Mercury, tungsten, and vanadium are alkali metals
False
True or false: Transition metals are generally gases at room temperature
False
True or false: all of the actinides have been found naturally on earth
False
True or false: the halogens are less reactive than metalloids?
False
The Group 17 element with the highest electronegativity is?
Fluorine (F)
Element with largest atomic radius
Francium (Fr)
Alkali Metals
Group 1 (except hydrogen), 1 valence electron in outer level, very reactive, soft, silver, shiny, low density; Lithium (Li), Sodium(Na), Potassium (k), Rubidium(Rb), Cesium(Cs), Francium (Fr). Never found in pure nature: they are too reactive Reactivity of these elements increased down the group
Halogens
Group 17 (7A) 7 valence electrons Never found in pure nature: they are too reactive F, Cl, Br, I, At In their pure form are diatomic molecules (F2, Cl2, Br2, I2) Ion: -1
noble gases
Group 18 (8A) 8 valence electrons (except helium; which only has 2) Only found pure in nature; they are chemically unreactive Colorless, odorless and unreactive; they were among the last of the natural elements to be discovered He, Ne, At, Kr, Xe, Rn, Uuo Ion: 0
alkaline earth metals
Group 2 2 valence electrons metallic elements harder than the alkali metals less reactive. Not found in pure nature: they are too reactive The word "alkaline" means basic Be, Mg, Cs, Sr, Ba, Ra
transition metals
Groups 3-12 Varying ionic charges Good conductors of electricity High luster when polished or cut Less reactive than s-block Most have high melting points Harder and more dense
Elements in the same column on the periodic table are said to be in the same?
Groups or family
Which noble gas has the highest first ionization energy?
Helium
Which Group 17 element has the least attraction for electrons?
I
Which element is member of the halogen family?
I
Which sequence correctly places the events in order of increasing ionization energy?
I ➡️ Br ➡️ Cl ➡️ F
isoelctronic ions
Iso: same Isoelectronic one have the same # of electrons Al+3, Mg+2, Na+1, Ne, F-1, O-2, N-3 All have 10 electrons All have the configuration 1s^2 2s^2 2p^6
inner transition metals
Lanthanides- Ce-Lu -Rare earths - shiny reactive metals Actinides- Ac-No -Unstable and radioactive
Who arranged the periodic table by atomic number? Also resolved discrepancies in Mendeleev's table
Moseley
Which of these elements has the least attraction for electrons in a chemical bond?
Nitrogen
The electron configuration ns^2np^6 represents which group of elements (n= energy level
Noble gas
Which element in Group 16 has the greatest tendency to gain electrons?
O
Which particle has a larger radius? S or S2-
S2-
ionization energy
The amount of energy required to remove an electron from an atom
As the elements Li to F in Period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the covalent radius of each successive element compare?
The relative electronegativity increases, and the atomic radius decreases.
Which is true of groups 3-12 on the periodic table?
They are able to conduct electricity
Which is true of halogens?
They are the most reactive of the metals They have seven electrons in their outer energy
True or false: The metalloids are in the p block of the periodic table
True
On the Periodic Table of the Elements, all the elements within Group 16 have the same number of
Valence electrons
Which electron configuration represents a transition element?
[Ar]3d^5 4s^2
Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having
a larger nuclear charge
The ability of carbon to attract electrons is
less than that of nitrogen and oxygen
Cations (+)
lose electrons Smaller bc they lose particles
What are the classes of elements?
metals: Everything to the LEFT of the stair step. nonmetals: Everything to the right of the stair step. metalloids: Elements bordering the stair step. (Except Al & Po) B, Si, Ge, As, Sb, Te, At
All of the group 18 elements besides helium are
noble gases and p-block elements
The elements calcium and strontium have similar chemical properties because they both have the same
number of valence electrons
Nonmetals
poor conductors of heat and electric current Tend to be brittle Many are gases at room temperature C, N, O, P, S, Se
electron affinity
the energy change that occurs when an electron is acquired by a neutral atom
Which statement best describes Group 2 elements as they are considered in order from top to bottom of the Periodic Table?
the number of principal energy levels increases, and the number of valence electrons remains the same
What is the periodic law?
the physical and chemical properties of the elements are periodic functions of their atomic numbers
An element with a partially filled d sub level in the ground state is classified as
transition metal
