Honors Chem Unit 5: Periodic Table
the name of group 1 on the periodic table:
alkali metals
Which has the largest atomic radius boron carbon aluminum silicon
aluminum
predicted properties of undiscovered elements:
mendeleev
Solid at room temp, ductile, malleable:
metal
anion
-negatively charged ion -formed when a nonmetal gains electrons
cation
-positively charged ion -formed when a metal loses electrons
Noble gases are ___ in electronegativity
0 -because they don't want to be in a compound
How many total electrons can occupy the 3d sublevel? a) 18 b) 10 c) 6 d) 32
10
Alkali metals are in which group of the periodic table? a) 1A or 1 b) 2A or 2 c) 7A or 17 d) 8A or 18
1A or 1
N is commonly used as
representation of any energy level
An element that has the electron configuration [Ne]3s23p5 is in Period 2 3 5 7
3
Halogens are located in which group of the periodic table a) 1A or 1 b) 2A or 2 c) 7A or 17 d) 8A or 18
7A or 17
Electronegativity
A measure of the ability of an atom in a chemical compound to attract electrons when the atom is in a compound
Choose the element with the higher first ionization energy Ca K Br
Br
Rank the following from lowest to highest ionization energy Br < Cl < F Cl < F < Br F < Cl < Br Br < F < Cl
Br < Cl < F
Of gallium, bromine and calcium, which has the highest electronegativity? Gallium Bromine Calcium
Bromine
Which of the following is the most electronegative? Cl Se Na I
Cl
Rank the following atoms in order from smallest to largest atomic radius Li < C < F C < F < Li F < Li < C F < C < Li
F < C < Li
1st ionization energy: smallest
Francium
Trends in atomic size: largest
Francium
columns on the periodic table:
Group
One of the least electronegative elements would be found on the periodic table in Group 1, Period 7 Group 3, Period 4 Group 5, Period 3 Group 17, Period 2
Group 1, Period 7
Which group has an element in each state of matter at room temperature? Group 1A Group 2A Group 7A Group 6A
Group 7A
Rank the following from lowest to highest electronegativity S < F < He He < S < F F < S < He He < F < S
He < S < F
1st ionization energy: largest
Helium
Trends in atomic size: smallest
Helium
Rank the following atoms in order from smallest to largest atomic radius Li < Na < K Na < K < Li K < Na < Li Li < K < Na
Li < Na < K
Choose the element with the higher first ionization energy Ca Ba Mg
Mg
Rank the atoms from lowest to highest ionization energy Mg < S < Si Si < S < Mg Mg < Si < S S < Si < Mg
Mg < Si < S
Which of the following sequences is correct for atomic size? Mg > Al > S Li > Na > K F > N > B F > Cl > Br
Mg > Al > S
Which is larger? Na Na⁺¹
Na
Which is larger? Na⁺ Mg²⁺
Na⁺
Mendeleev's periodic table did not list all elements in order of increasing atomic mass because he grouped together elements with similar a) properties b) atomic numbers c) names d) isotopes
a) properties
Group 18 (8A) on the periodic table:
Noble Gases
Which is larger? N³⁻ O²⁻ F⁻
N³⁻
Which is larger? O O⁻²
O⁻²
Which noble gas has the greatest atomic number Ar Xe Kr Rn
Rn
ionization energy
The amount of energy required to remove an (outer most layer) electron from an atom
Removing the outermost electron from a neutral atom involves the _____ of energy. absorption conversion release stability
absorption
The person whose work led to a periodic table based on increasing atomic number was a) Moseley b) Mendeleev c) Rutherford d) Cannizzaro
a) Moseley
These elements react most violently with water. a) alkalis b) halogens c) noble gases d) alkaline-earths
a) alkalis
What can be removed from an atom if ionization energy is supplied? a proton a neutron an electron an ion
an electron
An atom that has gained electrons and now has a negative charge is known as a molecule cation anion polyatomic ion
anion
Negatively charged ion:
anion
In nature, alkali metals are found only in compounds because they a) have small atoms b) are very reactive elements c) are rare elements d) each has a stable octet
are very reactive elements
Mendeleev arranged the elements in his periodic table in order of increasing a) atomic number b) number of protons c) number of electrons d) atomic mass
atomic mass
Which periodic trend generally decreases as you move from left to right across a period? ionization energy electronegativity atomic radius
atomic radius
On most periodic tables, the lanthanides and actinides appear a) on a separate page b) below the main portion c) on the back d) at the top
b) below the main portion
The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic a) masses b) numbers c) radii d) structures
b) numbers
Halogens are part of which block in the periodic table? a) d block b) p block c) s block d) f block
b) p block
Which one of the following is NOT a general property of metals? a) ductility b) poor conductor of heat and electricity c) malleability d) having a high luster
b) poor conductor of heat and electricity
The outer-level electron configuration of a neutral alkaline-earth metal atom consists of a) one electron in the s orbital b) two electrons in the s orbital c) one electron in the p orbital d) two electrons in the p orbital
b) two electrons in the s orbital
Which one of the following is incorrectly labeled? a) Ne, noble gas b) Cu, transition metal c) Ge, transition metal d) Cl, halogen
c) Ge, transition metal
An element found in groups 3-12 of the periodic table is classified as a(n) a) alkali metal b) alloy c) transition metal d) actinide
c) transition metal
Which type of element would have the following electron configuration: 1s²2s²2p⁶3s²3p⁶4s²3d⁴? a) alkali metal b) alkaline earth metal c) transition metal d) halogen
c) transition metal
Positively charged ion:
cation
Which of the following information about elements is usually NOT included in a periodic table? color symbol atomic number atomic mass
color
Transition metals are characterized as being different than representative elements because they have electrons in which orbitals? s p d f
d
What is the correct configuration for nickel, element 28? a) [Ar]4s²4p⁶5s² b) [Ar]4s²3d⁶ c) [Ar]3d¹⁰ d) [Ar]4s²3d⁸
d) [Ar]4s²3d⁸
The modern periodic table has elements arranged in order of a) colors b) melting and boiling points c) increasing atomic mass d) increasing atomic number
d) increasing atomic number
What two blocks compose the main group elements? a) p and d b) s and d c) f and d d) s and p
d) s and p
Mendeleev predicted that the gaps in his periodic table represented a) ions b) radioactive elements c) unstable elements d) undiscovered elements
d) undiscovered elements
The electrons that participate in bonding to form compounds are the _____ electrons. a) d-orbital b) f-orbital c) innermost d) valence
d) valence
Across a period in the periodic table, atomic radii generally decrease decrease, then increase increase increase, then decrease
decrease
Ionization energy tends to ______ as you move down a group. vary irregulary increase stay the same decrease
decrease
________ is the ability of an atom to attract electrons from another atom in a compound. ionization energy atomic radius ionic radius electronegativity
electronegativity
Electronegativity highest
fluorine
Which element is the most electronegative? fluorine carbon magnesium helium
fluorine
Which of the following has the highest electronegativity value? bromine chlorine fluorine
fluorine
Electronegativity lowest
francium
The atomic radius of an atom that is chemically bonded to an identical atom is equal to the distance between the nuclei half the distance between the nuclei twice the distance between the nuclei one-fourth the distance between the nuclei
half the distance between the nuclei
An element from which group is represented by an electron configuration that ends in ns²np⁵? a) alkaline-earth b) noble gas c) halogen d) alkali
halogen
Group 17 (7A) on the pt:
halogens
As the atomic numbers of the metals of Group 1 increase, the ionic radii: increase decrease remain the same cannot be determined
increase
Down a group in the periodic table, atomic radii generally decrease remain constant increase vary unpredictably
increase
Across a period in the periodic table, ionization energy generally decreases decreases, then increases increases remains constant
increases
As you move down a group, the atomic radius varies irregularly decreases remains the same increases
increases
Down a group in the periodic table, the change in ionization energy is due to increasing electron shielding decreasing charge of the nucleus increasing neutrons in the nucleus decreasing atomic radii
increasing electron shielding
The energy required to remove an electron from an element:
ionization
An anion gets _________ (explain)
larger -because you gain electrons causing more repulsion so the electron cloud spreads out -the higher the negative charge, the larger the ion
Block location for each element
last letter of electron configuration
Which has the largest atomic radius? carbon fluorine beryllium lithium
lithium
Metals tend to gain electrons to form cations gain electrons to form anions lose electrons to form anions lose electrons to form cations
lose electrons to form cations
A positive ion can be formed when an atom loses electrons gains protons loses protons gains electrons
loses electrons
Arranged elements by order of increasing atomic number
moseley
Which element would have the highest ionization energy? sodium calcium copper nitrogen
nitrogen
atomic radius
one-half the distance between the nuclei of identical atoms that are bonded together
Which of the following elements would have an ion that is larger than its neutral atom? sodium magnesium copper oxygen
oxygen
rows on the periodic table:
periods
Which element would be most likely to both gain and lose electrons easily? a) oxygen b) silver c) neon d) silicon
silicon
Trends in atomic size/radius: going from left to right
size generally decreases
Trends in atomic size/raidus: up to down
size generally increases
A cation gets ______ (explain)
smaller -because you lose the valance electrons -remaining electrons are drawn closer (more attracted) to the nucleus by its unbalanced positive charge -the higher the charge, the smaller the ion
Which element is most likely to form a cation? sodium helium oxygen fluorine
sodium
Which has the smallest atomic radius? magnesium silicon sulfur sodium
sulfur
An element has a low ionization energy and electronegativity. It has relatively low reactivity with oxygen and water and is an excellent conductor of electricity. What is this element? transition metal halogen noble gas alkali metal
transition metal
An electron that is in the highest energy level of an atom and determines the atom's chemical properties is called a(n) paired electron extra electron opposite-spin electron valence electron
valence electron
Elements in Group 18 have very low reactivity good conductivity very high reactivity metallic character
very low reactivity
the remaining electrons are sucked closer to each other when
you lose more electrons
