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Which element has the greatest electronegativity?


what are the group one metals known as?

alkali metals

the electron configuration of aluminum , atomic number 13, is [Ne] 3s2 3p1. What period is Aluminum in?


the periodic law states that the properties of elements are periodic functions of their atomic numbers. This means that the ____ determines the position of each element in the periodic table.

number of protons

Which orbitals are characteristic of the lanthanide elements?

f orbitals

The electron configuration of an element is [Kr] 4d6 5s1. To what group does this element belong?

Group 7

The electron configurations of the noble gases from neon to radon in the periodic table end with filled ___

p orbitals

if n stands for the highest occupied energy level, the outer configuration for all Group 1 elements is ___


Because the first energy level only the 1s sublevel, the number of elements in this period is


the first electrons to be removed when d-block elements form ions are the ___

s electrons

Ionization energy is the energy required to remove _______ from an atom of an element

an electron

Neutral atoms with a s2p6 electron configuration in the highest energy level are best classified as ____


Mendeleev is credited with developing the first successful _____

periodic table

The energy required to remove an electron from an atom _____ as you move left to right from K through Fe

generally increases

Among the d-block elements, as atomic radii decrease, electronegativity values ____


Elements in the d- sublevel is being filled have the properties of ___


a horizontal row of blocks in the periodic table is called a ___


In a row in the periodic table, as the atomic number increases, the atomic radius generally ____


The most useful source of general informantion about the elements for anyone associated with chemistry a ____

periodic table

the electrons available to be lost, gained, or shared, when the atoms form molecules are called ___

valence electrons

Across a period, the atomic radii of d-block elements generally___


Identify the sublevels in a periodic period that contain 32 elements


which groups in the main group have lower electronegativity than d-block elements?

groups 1 and 2

The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to ____


A positive ion is known as a ___


The person whose work led to a periodic table based on an increasing atomic number was _____


Nitrogen electron configuration is 1s2 2s2 2p3. To what group does N belong?


the energy required to remove an electron from an atom is the atoms

ionization energy

the ionization energies for removing successive electrons from Na are 496 kJ/MOL, 4562 KJ/MOL, 6012 Kj/MOL, and 9544 kJ/MOL. the great jump in ionization energy after the first electron is removed indicates that ___

the noble gas configuration has been reached

for each successive electron removed from an atom, the ionization energy ___


a neutral atom that represents aquiring an electron in an exothermic process is

A + e- > A- + energy

what are the radioactive elements with atomic numbers from 90-103 in the periodic tabble called


the elements whose electron configuration n with s2p5 in the highest occupied energy level belong to ____


bromine, atomic number 35, belongs to group 17. how many electrons does bromine have in its outermost energy level?


the periodic law allows some properties of an element to be predicted on its ____

position in the periodic table

group 2 elements, the valence electrons are in sublevel ____


In period 3 there are 8 elements. What sublevels are being filled?

s and p

the number of valence electrons in group 2 elements is ____


Argon, Krypton, and Xenon are ____

noble gases

what are the elements with atomic numbers 58--71 in the periodic table called?


for groups 13-18, the total number of electrons in the highest occupied level equals the group number ___

minus 10

with a group of elements, as the atomic number increases, the atomic radius ____


compared to the alkali metals, the alkaline-earth metals are _____

less reactive

a negative ion is know as an___


when determining the size of an atom, by measureing the distance between identical adjacent nuclei, the radius of an atom is ____

half the distance between nuclei

Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing

atomic mass

the most characteristic property of the noble gases is that they ___

are largely unreactive

elements in a group or column in a periodic table can be expected to have similar ___


in the modern periodic table, elements are ordered according to ___

increasing atomic number

the most reactive group on nonmetals are the ___


in which of these compounds is the bond between the atoms not a nonpolar covalent bond?


The b-f bond in bf3 (electronegativity for b is 2.0; electronegativity for f is 4.0) is


a chemical bond formed by the attraction between positive ions an surrounding mobile is a ___

metallic bond

a chemical bond resulting from the electrostatic attraction between positive and negative ions is called an____

ionic bond

the electron-c model of bonding represents ___

metallic bonding

in drawing a lewis structure , each nonmetal atom except hydrogen should be surronded by _____

8 electrons

if the lattic energy compound A is greater than that of compound B ____

the bonds in compound A are stronger

the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of eqaul energies is called


lattice energy is the energy released in the formation of a ____

ionic compound

if two covalently bonded atoms are identical, the bond is ___

nonpolar covalent

in many compounds, atoms of main-group elements form bonds so that the number of electrons in the outermost energy levels of each atom is


the electrons involved in the formation of a chemical bond are called

valence electrons

according to VSEPR theory, the shape of an ab3 molecule is

triangular planar

nonpolar covalent bonds are not common because

1 atom usually attracts electrons more strongly than the other

the intermolecular attraction between a hydrogen atom bonded to a strongly electronegative atom and the unshared pair of electrons of another strongly electronegative atom is called

hydrogen bonding

the model for predicting the shape of a molecule that is based on the repulsion of the electrons for each other is called

VSEPR theory

in drawing a lewis structure the central atom is the

least electronegative atom

the ions in an ionic compound are organized into a


bond length is

the separation for which potential energy is at a minimum

compared with ionic compounds, molecular compounds ___

have lower melting points

mulitiple covalent bonds occur in atoms that contain carbon, nitrogen, or


to draw a lewis structure, it is not necessary to know

bond energies

according to the VSEPR theory, an ab2 molecule is


a molecule is a

neutral group of atoms held together by covalent bonds

the greater the electronegativity difference between two bonded atoms, the greater percentage of

ionic character

a polar molecule contains

a region of positive charge and a region of negative charge

use VSEPR theory to predict the shape of the hydrogen sulfide model, H2S


a bond that is less than 5% ionic is considered

nonpolar covalent

which of the following is not a property of an ionic compound?

low boiling point

the chemical bond formed when two atoms share electrons is called a

covalent bond

a ____ shows the types and numbers of atoms joined in a single molecule of a molecular compound

molecular formula

the octect rule states that chemical compounds tend to form so that each atom has an octet of electrons in the

highest occupied energy level

the substance who lewis structure shows three covalent bonds is


if a material can be shaped or extended by physical pressure, such as hammering which property does the material have?


how many extra electrons are in the lewis structure of the phosphate ion, PO4 -3


the weak intermolecular forces resulting from instantaneous and induced dipoles are called

londen dispersion forces

shifting the layers of an ionic crystal causes the crytal to


the equal and opposite charges present in two regions of a polar molecule create a


the electron configuration of nitrogen is 1s2 2s2 2p3. How many more electrons does N need to satisfy the octet rule?


which of the following is not an example of a molecular formula?


atoms naturally move

toward low potential energy

metals are malleable because the metallic bonding

allows one plain of ions to slide past another

in metals, the valence electrons

are shared by all the atoms

bonding in molecules or ions that cannot be correctly represented by a single lewis structure is


ionic compounds are brittle because the strong attractive forces

hold the layers in relatively fixed positions

the concept that electrostatic repulsion between electron pairs surrounding an atom causes these pairs to be separated as far as possible is the foundation of

the VSEPR theory

a shorthand representation of the compostion of a substance using atomic symbols and numerical subscripts is called a

chemical formula

a formula that shows types and numbers of atoms combined in a single molecule is called a

molecular formula

compared with the energies of neutral atoms, a crystal lattice has

lower potential energy

which hybrid orbitals help explain how methane bonds?

sp3 orbitals

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