chemistry 1201 exam 2 Dr. Borill

decreases, increases

-First IE _______ down the group in the periodic table because electrons in the outermost principal level are increasingly farther away from the positively charged nucleus and are therefore held less tightly. -First IE generally _______ across the period in the periodic table because electrons in the outermost principal energy level experience a greater effective nuclear charge

molecular model

A ___________ is a more accurate and complete way to specify a compound.

structural formula

A ___________ is a ~sketch or ~diagram of how the atoms in the molecule are bonded to each other. -communicates the most information. -It conveys the type and actual number as well as the arrangement of the atoms in the molecule. -It's a "visual" picture of the compound.

molecular formula

A ____________ gives the ~actual~ number of atoms of each element in a molecule of a compound. -It does not tell you how each of the atoms are bonded to each other.

ball-and-stick molecular model

A _____________ represents atoms as balls and chemical bonds as sticks; how the two connect reflects a molecule's shape.

electron configuration.

A description of the orbitals occupied by electrons is called an ____________

empirical formula

An ___________ gives the ~relative~ number of atoms of each element in a compound. It is the simplest whole-number (ratio) representation of the type and number of elements present in a molecule.

decreases

Atomic radius ________ across a period (left to right) -Adding electrons to the same valence shell -Effective nuclear charge increases across a period. -Valence shell held closer

increases

Atomic radius ________ down a group. -Valence shell farther distance from nucleus -Effective nuclear charge decreases as you go down a column.

smaller

Cation radius is ________ than its corresponding atom radius

Empirical formula Molecular formula Structural formula

Chemical formulas can generally be categorized into three different types:

groups , family

Columns in the table are referred to as ______ or a ________.

chemical bonds.

Compounds are composed of atoms held together by __________

halogens

Contains nonmetals, (F, Cl, Br, I, At) 7 valence electrons in it's outermost energy level (1 fewer than the next noble gas). Very reactive

attractions, repulsions

Coulomb's law describes the ________ and _________ between charged particles.

Periodic

Density, along with other properties such as atomic radii, is a _________ property of matter.

diamagnetism

Electron configurations that result in all paired electrons mean that the atom or ion will have no magnetic field; this is called ____________. Slightly repelled by a magnetic field

paramagnetism

Electron configurations that result in unpaired electrons mean that the atom or ion will have a net magnetic field; this is called ________________. Will be attracted to a magnetic field

aufbau principle.

Electrons enter (e.g., fill) atomic orbitals from lowest energy to highest:

s, p

Electrons in __ orbitals are better shielders than electrons in ____ orbitals.

core (inner) electrons.

Electrons in lower-energy shells are called _______________

similar

Elements in a group or family have ________ properties.

Metals Nonmetals Metalloids

Elements in the periodic table are classified as the following:

metals

Except for the noble gases, _______ generally have smaller first ionization energies and nonmetals generally have larger electron affinities.

energy to remove electron from neutral atom

First ionization energy =

multi-electron

For _____________ atoms (all others but the H atom), the equation cannot be exactly solved because of the electron-electron interactions that happen between two electrons.

positive

For like charges, the potential energy (E) is _______ and decreases as the particles get farther apart as r increases.

interaction, shielding, penetration

For multi-electron atoms, the energies of the sublevels are split. Caused by charge _________, ____________, and _________

negative

For opposite charges, the potential energy is___________ and becomes more negative as the particles get closer together

space-filling molecular model

In a _________________, atoms fill the space between each other to more closely represent our best estimates for how a molecule might appear if scaled to visible size.

shielding

In a multi-electron atom, each electron experiences both an attraction to the protons in the nucleus and the repulsion by other electrons in the atom. These repulsions cause an electron to experience a net reduction in attraction to the nucleus. We refer to this as ___________

increases

Ion size ________ down the column.

charge

Ions in the same group have the same ____________.

endothermic

It is an ___________ process (requires the input of energy to remove the electron). Valence electron easiest to remove, lowest IE

Electron Affinity

It is the energy associated with the addition of an electron to the valence shell of an atom that is in the gas phase.

Ionization Energy (IE)

It is the ~minimum energy needed~ to remove an electron from an atom or ion in the gas phase.

columns

Mendeleev arranged the rows so that elements with similar properties would fall within the same vertical _______.

Quantum theory

Mendeleev's periodic law predicts patterns but does NOT explain why the patterns or similarity in properties occurs. ______________ explains the why.

decreases , increases

Metallic character __________left to right across a period. Metallic character __________ down the column

cations, anions

Metalloids can either lose electron(s) from p and then s orbitals to form __________ or gain electrons in their p orbitals to form ________.

metallic, nonmetallic

Metalloids in chemical reactions can exhibit ______ or__________ behaviors.

cations

Metals form ______

compounds

Molecules are __________

anions

Nonmetals form ________

half-arrow

Orbital diagrams use a square to represent each orbital and a __________ to represent each electron in the orbital

Pauli exclusion principle.

Orbitals that are in the same sublevel have the same energy . There can be no more than two electrons per orbital.

degenerate

Orbitals with the same energy (E) are said to be _________.

diamagnetic

Paired spins are ___________.

INCREASES, DECREASES

Periodic Trend: Effective nuclear charge ________ as you go across a period and _________ as you descend down a column.

physical and chemical

Reoccurring patterns in the _______ and _______ properties of elements aid scientists in predicting undiscovered elements and understanding elemental behavior.

periods

Rows of the periodic table are referred to as ________.

energy to remove from 1+ ion, etc.

Second IE =

cancel

Spins must ______ in an orbital

larger

The _______ the effective nuclear charge on the electron to be removed, the more energy it takes to remove it.

mass-to-volume (density)

The __________ ratio of atoms increases as you move down a column of elements.

effective nuclear charge

The _______________ is a net positive charge that is attracting a particular electron.

molecular compounds

The covalently bound atoms compose a molecule. Hence, they are referred to as :

penetration

The degree of __________ is related to the orbital's radial distribution function.

spin quantum number, ms.

The electron's spin adds a fourth quantum number to the description of electrons in an atom, called the ____________

valence electrons.

The electrons in all the sublevels with the highest principal energy shell (level) are called the __________

stronger

The larger the effective nuclear charge an electron experiences, the _________ the attraction it will have for the nucleus.

larger

The loss of electrons results in the remaining electrons in the atom experiencing a _________effective nuclear charge than the neutral atom.

less

The lower the value of the l quantum number (orbital quantum number), the ______ energy the sublevel has.

eight

The noble gases have _______ valence electrons

distance the valence electrons are from the nucleus.

The size of an atom is related to:

effective nuclear charge

The total amount of attraction that an electron feels for the nucleus's protons is called the __________________(Zeff) of the electron.

farther

The_________ the electron most probably is from the nucleus, the less energy it takes to remove it.

nonbonding bonding radius

There are several methods for measuring the radius of an atom, and they give slightly different numbers. Van der Waals radius = ____________ Covalent radius = __________

smaller effective nuclear charge

These "new valence electrons" experience a ___________________ than the "old valence electrons."

Transition and Inner Transition Metals:

They are located in the d-block area of the periodic table. In chemical reactions, they will lose electron(s) from s and then d orbitals to form cations.

p-block Metals

They are located in the p-block area (left-hand side of the metalloids) of the periodic table. In chemical reactions, they will lose electrons from the s and p orbitals to form cations.

Nonmetals

They are located in the upper right-hand side of the periodic table. p-block area

Alkali Metals

They have one more electron than the previous noble gas and occupy the first column. In their reactions, they lose one electron, and the resulting electron configuration is the same as that of a noble gas. Forming a cation with a 1+ charge

Alkaline Earth Metals:

They have two more electrons than the previous noble gas and occupy the second column. In their reactions, they lose two electrons, and the resulting electron configuration is the same as that of a noble gas. Forming a cation with a 2+ charge

sharing

They involve the ________ of electrons between two atoms.

exhibit a repeating pattern.

To be periodic means to -___________

electron spin , energy splitting of sublevels.

Two additional concepts affect multi-electron atoms: __________ and ________________

The Lewis Model

Valence electrons are represented as dots.

added

When atoms form anions, electrons are ________ to the valence shell.

Hund's Rule

When filling orbitals that have the same energy (degenerate), place one electron in each orbital before completing pairs.

increasing mass

When the elements are arranged in order of____________, certain sets of properties recur periodically.

entirely new

When two or more elements combine to form a compound, an _________substance results.

molecule

When two or more elements combine, a _______ is formed.

(c) the valence electrons in S

Which atom's valence electrons experience the greatest effective nuclear charge? (a) the valence electrons in Mg (b) the valence electrons in Al (c) the valence electrons in S

Z, S

___ is the nuclear charge, and ___ is the number of electrons in lower energy levels.

Spin

________ is a fundamental property of all electrons.

transition, inner transition, transition

___________ elements and ____________ metals or ________metals: properties tend to be less predictable based simply on their position in the periodic table. In the periodic table, this area is labeled by a number and the letter B.

Ionic bonds

___________ occur between metals and nonmetals.

Metallic

____________ elements make up the majority of the elements in the periodic table

main-group

____________ elements: properties tend to be largely predictable based on their position in the periodic table. In the periodic table, this area is labeled by a number and the letter A.

Metallic character

____________ is how closely an element's properties match the ideal properties of a metal. More malleable and ductile, better conductor, and easier to ionize

Metalloids

are located in the p-block area of the periodic table between the metal and nonmetal elements. Sitting on the "steps" of the zigzag diagonal line indicatedon the periodic table

chemical formula.

compound is represented by its _______

Halogens

have the highest EA for any period

electrons

ionic bonds involve the transfer of _______ from one atom to another.

oxidized

metals Lose electrons in reactions—_______

nonreactive

noble gases are especially

reduced//reduction

nonmetals Gain electrons in reactions—_________

Covalent bonds

occur between two or more nonmetals.

1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p

orbitals fill in the following order: