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