Which element has the greatest electronegativity?
what are the group one metals known as?
the electron configuration of aluminum , atomic number 13, is [Ne] 3s2 3p1. What period is Aluminum in?
number of protons
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.
Which orbitals are characteristic of the lanthanide elements?
The electron configuration of an element is [Kr] 4d6 5s1. To what group does this element belong?
The electron configurations of the noble gases from neon to radon in the periodic table end with filled ___
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 ___
Ionization energy is the energy required to remove _______ from an atom of an element
Neutral atoms with a s2p6 electron configuration in the highest energy level are best classified as ____
Mendeleev is credited with developing the first successful _____
The energy required to remove an electron from an atom _____ as you move left to right from K through Fe
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 ____
the electrons available to be lost, gained, or shared, when the atoms form molecules are called ___
Across a period, the atomic radii of d-block elements generally___
Identify the sublevels in a periodic period that contain 32 elements
groups 1 and 2
which groups in the main group have lower electronegativity than d-block elements?
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
the noble gas configuration has been reached
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 ___
for each successive electron removed from an atom, the ionization energy ___
A + e- > A- + energy
a neutral atom that represents aquiring an electron in an exothermic process is
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?
position in the periodic table
the periodic law allows some properties of an element to be predicted on its ____
group 2 elements, the valence electrons are in sublevel ____
s and p
In period 3 there are 8 elements. What sublevels are being filled?
the number of valence electrons in group 2 elements is ____
Argon, Krypton, and Xenon are ____
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 ___
with a group of elements, as the atomic number increases, the atomic radius ____
compared to the alkali metals, the alkaline-earth metals are _____
a negative ion is know as an___
half the distance between nuclei
when determining the size of an atom, by measureing the distance between identical adjacent nuclei, the radius of an atom is ____
Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing
are largely unreactive
the most characteristic property of the noble gases is that they ___
elements in a group or column in a periodic table can be expected to have similar ___
increasing atomic number
in the modern periodic table, elements are ordered according to ___
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 ___
a chemical bond resulting from the electrostatic attraction between positive and negative ions is called an____
the electron-c model of bonding represents ___
in drawing a lewis structure , each nonmetal atom except hydrogen should be surronded by _____
the bonds in compound A are stronger
if the lattic energy compound A is greater than that of compound B ____
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 ____
if two covalently bonded atoms are identical, the bond is ___
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
according to VSEPR theory, the shape of an ab3 molecule is
1 atom usually attracts electrons more strongly than the other
nonpolar covalent bonds are not common because
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
the model for predicting the shape of a molecule that is based on the repulsion of the electrons for each other is called
least electronegative atom
in drawing a lewis structure the central atom is the
the ions in an ionic compound are organized into a
the separation for which potential energy is at a minimum
bond length is
have lower melting points
compared with ionic compounds, molecular compounds ___
mulitiple covalent bonds occur in atoms that contain carbon, nitrogen, or
to draw a lewis structure, it is not necessary to know
according to the VSEPR theory, an ab2 molecule is
neutral group of atoms held together by covalent bonds
a molecule is a
the greater the electronegativity difference between two bonded atoms, the greater percentage of
a region of positive charge and a region of negative charge
a polar molecule contains
use VSEPR theory to predict the shape of the hydrogen sulfide model, H2S
a bond that is less than 5% ionic is considered
low boiling point
which of the following is not a property of an ionic compound?
the chemical bond formed when two atoms share electrons is called a
a ____ shows the types and numbers of atoms joined in a single molecule of a molecular compound
highest occupied energy level
the octect rule states that chemical compounds tend to form so that each atom has an octet of electrons in the
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
londen dispersion forces
the weak intermolecular forces resulting from instantaneous and induced dipoles are called
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?
toward low potential energy
atoms naturally move
allows one plain of ions to slide past another
metals are malleable because the metallic bonding
are shared by all the atoms
in metals, the valence electrons
bonding in molecules or ions that cannot be correctly represented by a single lewis structure is
hold the layers in relatively fixed positions
ionic compounds are brittle because the strong attractive forces
the VSEPR theory
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
a shorthand representation of the compostion of a substance using atomic symbols and numerical subscripts is called a
a formula that shows types and numbers of atoms combined in a single molecule is called a
lower potential energy
compared with the energies of neutral atoms, a crystal lattice has
which hybrid orbitals help explain how methane bonds?