Honors Chemistry Quarter 2 Exam: Units 4-6

What is the difference between "white" light and blue or red light? -"White" light has all the wavelengths of the visible spectrum, red and blue light have specific wavelengths. -Red and blue light have all the wavelengths of the visible spectrum, "white" light has specific wavelengths.

"White" light has all the wavelengths of the visible spectrum, red and blue light have specific wavelengths.

What is the maximum number of electrons that can occupy the 5d subshells?

(up to) 10 electrons

What is Li core charge

+1

What is the core charge of a Hydrogen atom?

+1 (one valence electron)

What is He core charge?

+2

The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively? -+5 and +8 -+3 and +6 -+5 and +6 -+3 and +8 -+1 and +4

+3 and +6 (EXPLANATION:The valence electrons in an oxygen atom are attracted to the nucleus by a positive charge nearly double that of boron. Therefore, the electrons in oxygen are held closer to the nucleus, giving it a smaller radius.)

What is Cl core charge

+7

What is the core charge of a fluorine atom?

+7 (7 valence electrons: look at group number, count 1,2-3,4,5,6,7)

Know the resonance structures for CO₃²⁻ and its formal charges

- charge on 2 of the Os with 6 dots -the C-O bond order is 4/3 (1.5)

What is the formal charge of the last N: HN₃? (quiz question)

-1 (5-6=-1)

trigonal bipyramidal

-120 and 90 degrees -see-saw shaped -T shaped -linear

How can you find valence electrons? and what are they?

-Electrons in the outermost orbital -you can find them by look at groups in the periodic table skipping the transition metals (1-7,8)

When an electron drops to a lower energy level, it gains energy. (T/F)

-F (it has to lose some of its energy to move)

Identify two elements that can represent "X" if X has one lone pair in the molecule XBr₄?

-There are 28 total valence electrons for Br and since X has one pair of lone electrons so now the total is 34 electrons -Se, Te can work because it can hold more than 8 valence electrons

The condensed electron configuration of sulfur, element 16, is __________. -[He] 2s⁴, 2p⁸ -[Ne] 3s², 3p⁴ -[Ne} 3s²

-[Ne] 3s², 3p⁴

When do you not include formal charges?

-when they are all zero -or when it's neutral

Electron Configuration by group

..

Electron Configuration on periodic table

...

HCN dipole moment

... polar

Calcium has __ unpaired electrons

0

For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity? (quiz) -1 -2 -1 or 2 -3 -1 or 3

1

Ga has __ unpaired electron(s)

1

How many UNPAIRED electrons are in the ground state electron configuration for boron? -0 -1 -2 -3 -4 -5 -6

1

There are __________ unpaired electrons in a ground state chlorine atom. >1 >4 >0 >3

1

What is the bond order for H₂

1 (H-H, there is one bond, and the bond energy is 436 kJ/mole)

Rank types of electromagnetic radiation from highest to lowest frequency. -Cell phone -UV radiation from a halogen light bulb -infrared radiation for a scanner

1-UV radiation from a halogen light bulb 2-infrared radiation for a scanner 3-Cell phone (TIP-The energy of electromagnetic waves is directly proportional to the frequency of that wave; the higher the energy of a wave, the higher the frequency. The wave equation is c=λν, where λ is the wavelength of the wave and ν is the frequency of the wave. Therefore, frequency is inversely proportional to wavelength but proportional to energy.)

phosphorus has __ core electrons, _ valence electrons, and _ unpaired electrons in the ground state.

10, 5, 3

The F-N-F bond angle in the NF3 molecule is slightly less than __________. -120 -109.5 -180

109.5

What is the value of the bond angles in CH4 (enter bond angle) (tetrahedral)

109.5

Tetrahedral

109.5 degrees (like CH4)

How many valence electrons does H₂CO have?

12

The O-S-O bond angle in is slightly less than __________. -180° -90° -60° -120° -109.5°

120

What is the approximate bond angle in BCI3? -180 -120 -109.5 -107 -104.5

120

What is the value of the bond angles in BF3? Enter the bond angle of the molecule.

120

The O-C-O bond angle in the CO3 2- ion is approximately __________. -90 degrees -120 degrees -180 degrees -109.5 degrees

120 degrees

Trigonal planar

120 degrees

PI3Br2 is a nonpolar molecule. Based on this information, determine the I−P−I bond angle, the Br−P−Br bond angle, and the I−P−Br bond angle. Enter the number of degrees of the I−P−I, Br−P−Br, and I−P−Br bond angles, separated by commas (e.g., 30,45,90)

120, 180, 90

How many valence electron are in F₂?

14 (7+7)

How many valence electrons does Cl₂ atom have?

14 (7+7)

What is the maximum number of electrons that can occupy the f subshells?

14 electrons (7 orbitals)

The typical bond length for a C-N single bond (bond order=1) is 147 pm. Based on this result, what is the expected typical bond length for a C-O single bond (Bond order=1) (quiz question) A) 143 pm B)147 pm C) 151 pm D) 205 pm

143 pm

How many valence electrons are in HCOOH? (quiz question)

18 (2+4+12)

What is the value of the bond angle in XeCl2? (linear) Enter the bond angle of the molecule.

180

Which one of the following configurations depicts an excited oxygen atom? -1s², 2s², 2p⁴ -1s², 2s², 2p², 3s²

1s², 2s², 2p², 3s²

The complete electron configuration of vanadium, element 23, is __________. -1s⁴, 2s⁴, 2p⁸, 3s⁴, 3p³ -1s², 2s², 2p⁶, 3s², 3p⁶, 3d³, 4s²

1s², 2s², 2p⁶, 3s², 3p⁶, 3d³, 4s²

Arsenic electron configuration

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p³

The ground state electron configuration of Ga is __________. -[Ar] 4s², 3d¹¹ -1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p¹

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p¹

**How many UNPAIRED electrons are in the ground state electron configuration for carbon? -0 -1 -2 -3 -4 -5 -6

2

CIF3 has "T-shaped" geometry. How many nonbonding domains are in this molecule? -0 -1 -2 -3 -4

2

ClF3 has "T-shaped" geometry. There are __________ non-bonding domains in this molecule. -0 -1 -2 -3 -4

2

Hydrogen must share ___ electrons (bonding pair)

2

Indicate how many unpaired electrons the Pt atom has.

2

The 3p subshell in the ground state of atomic silicon contains __________ electrons. -36 -10 -6 -2 -8

2

What is the bond order for CO₂?

2 (the bond energy is 804)

What is the maximum number of electrons that can occupy the 2s subshells?

2 electrons (1 orbital)

Hydrogen must share ___ ____ or a ____ _____

2 electrons, bonding pair (which is represented by a line, and no more than 1 line)

carbon has_ core electrons, _ valence electrons, and _ unpaired electrons in the ground state.

2, 4, 2

neon has _ core electrons, _ valence electrons, and _ unpaired electrons in ground state

2, 8, 0

The central Xe atom in the XeF4 molecule has __________ unbonded electron pairs and __________ bonded electron pairs in its valence shell.

2,4

(quiz question) How many valence electrons are there in the PCl₃ molecule?

26 (5+7(3))

When electrons are removed from a lithium atom they are removed first from which orbital?

2s

(quiz) Using the periodic table, identify which set of electron sublevels is NOT organized from lowest energy to highest energy. -2s, 2p, 3s, 3p, 3d, 4s -1s, 2s, 2p, 3s, 3p, 4s -2s, 2p, 3s, 3p, 4s, 3d -5s, 4d, 5p, 6s, 4f, 5d

2s, 2p, 3s, 3p, 3d, 4s

What is the bond order of N₂?

3 (bond energy is 945)

T-Shaped

3 bonds, 2 lone pairs (90 degrees)

How many valence electrons are in C₆H₆? (quiz question)

30 (24+6)

How many valence electrons are in SO₄⁻² (quiz question)

32 (6+24+2)

How many valence electrons does SiCl₄

32 [4+7(4)=32]

Which group in the periodic table contains elements with the valence electron configuration of ns² np¹? -1A -4A -8A 7A -3A

3A

*The elements in the __________ period of the periodic table have a core-electron configuration that is the same as the electron configuration of neon. -1s -2nd -3rd -4th -5th

3rd

How to calculate bond order if you have renocence structures? -What is Carbonate (CO₃²⁻) bond order

4/3 (represented as fraction: there are 4 bonds in one structure averaged over 3 structures)

The visible light spectrum covers the wavelength range ________. -400 to 700 nm -250 to 400 nm -1400 to 2000 nm -700 to 900 nm

400 to 700nm

In a ground-state silver atoms, the __________ subshell is partially filled. -3d -3s -4d -4p -4s

4d

The largest principal quantum number in the ground state electron configuration of iodine is __________. -4 -7 -6 -1 -5

5

PCI5 has ________ electron domains and a ________ molecular arrangement. -5, square pyramidal -6, seesaw -6, trigonal bipyramidal -6, tetrahedral -5, trigonal bipyramidal

5, trigonal bipyramidal

PCl5 has __________ electron domains and a __________ molecular arrangement.

5, trigonal bipyramidal

Formal Charge of NH₄⁺?

5-4=+1 for N (So formal charge is # of valence electrons - # of valence electrons in the bonded atom, so count the lines)

elements that have 3 unpaired electrons are where in the periodic table (name group)

5a ????

The 3p subshell in the ground state of atomic xenon contains __________ electrons. -8 -10 -36 -6 -2

6

What is the maximum number of electrons that can occupy the 3p subshells?

6 electrons

How many valence electrons are in C₆H₁₂O₆? (quiz question)

72 (24+12+36)

How many valence electrons does SiH₄ molecule have?

8

The second shell in the ground state of atomic argon contains __________ electrons. -2 -6 -8 -18 -36

8

How many valence electrons are in NH₄⁺ (quiz question)

8 (5+4-1)

Elements in group __________ have a np6 electron configuration in the outer shell. -4A -^A -5A -7A -8A

8A

What is the value of the smallest bond angle in IF4−? (square planar Enter the smallest bond angle of the molecule.

90

octahedral (square pyramidal, square planar)

90

What is the Lewis structure for HSH and HOH? Is the S-H bond weaker than the O-H bond on HOH? (quiz question)

>> H-S-H (with 2 dots above and below S) >> H-O-H (with 2 dots above and below O) >S-H is the weaker bond

Phase Change Diagram (test objective)

A diagram that shows a physical change of a substance because of a temperature change (as time goes on by the minute)

Which equation correctly represents the first ionization of aluminum? =Al(g)→Al+(g)+e− =Al(g)→Al−(g)+e− =Al+(g)+e−→Al(g)

Al(g)→Al+(g)+e−

__________ have the lowest first ionization energies of the groups listed. -Noble gases -Alkaline earth metals -Halogens -Transition elements -Alkali metals

Alkali metals (Fr)

Of the choices below, which gives the order for first ionization energies? -Cl > S > Al > Ar > Si -Al > Si > S > Cl > Ar -S > Si > Cl > Al > Ar -Ar > Cl > S > Si > Al

Ar > Cl > S > Si > Al

Of the choices below, which gives the order for first ionization energies? -Cl > S > Al > Ar > Si -Ar > Cl > S > Si > Al -Al > Si > S > Cl > Ar -S > Si > Cl > Al > Ar -Cl > S > Al > Si > Ar

Ar > Cl > S > Si > Al

Which has the highest electronegativity? Zn, Ge, Ga , As.

As

Of the molecules below, only___ is polar (quiz) -CH4 -SbF5 -AsH3 -SF6 -I2

AsH3

Which element fits the following description: an element hat has 3 electrons in the n=2 energy level (QUIZ**) -Al -B -Be -Ga -Mg -Na

B

Of the following species, __________ will have bond angles of 120°. -PH3 -NCl3 -ClF3 -BCl3

BCl3 (trigonal planar)

4 domains

Based on the structure, how many electron domains surround the C atom in this molecule?

Cu

Based on their positions in the periodic table, predict which atom of the following pair will have the smaller first ionization energy: Fe, Cu (Same row)

Sb

Based on their positions in the periodic table, predict which atom of the following pair will have the smaller first ionization energy: P, Sb

Pb

Based on their positions in the periodic table, predict which atom of the following pair will have the smaller first ionization energy: Pb, Hg

Cl

Based on their positions in the periodic table, predict which atom of the following pair will have the smaller first ionization energy: Cl, Ar

1s², 2s² is what element

Be

____ _____ is defined as the energy required to break the the bond that holds two adjacent atoms together in a molecule

Bond energy

What elements follow the octet rule?

C, N, O, F

What is the bond order for the C-C and C-H bond of H₃CCH₃

C-C=1 C-H=1

Which bond is the shortest? (quiz question) *C-Cl *C-F *C-Br *C-I

C-F (is also the strongest bond b/c the low number of electrons which make it close to its atomic radius. This results is it being the strongest and the shortest)

Which bond is the weakest? (quiz question) *C-Cl *C-F *C-Br *C-I

C-I (is also the longest b/c the high amount of electrons make it very far away from its atomic radii, which makes it spread out and very weak)

Example of a nonpolar molecule

CO2

How can you use the shape of a molecule to determine its polarity?

Center atom: -no lone pairs= nonpolar -lone pairs= polar

Of the molecules below, only ____ is nonpolar. -Co2 -H2O -NH3 -TeCl2 -HCl

Co2

[Ar] 4s¹ 3d⁵ is what element

Cr

Place the following elements in order of decreasing atomic size: lead, phosphorus, oxygen, cesium, barium, and silicon. (largest to smallest_

Cs, Ba, Pb, Si, P, O

Which statement best describes the polarity of SF4I2? -The molecule is always polar. -The molecule is always nonpolar. -Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar.

Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar

Has the highest electronegativity?

F (Fluorine)

Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? -F < O < S < Ba < Mg -F < O < S < Mg < Ba -F < S < O < Mg < Ba -O < F < S < Mg < Ba

F < O < S < Mg < Ba

Which atom has the highest electronegativity? Si or F?

F-4.19 (while Si= 1.92)

linear or bent

For a molecule with the formula AB2 the molecular shape is __________. -linear or trigonal planar -linear or bent -T-shaped -trigonal planar -linear or T-shaped

trigonal planar, trigonal pyramidal, or T-shaped

For a molecule with the formula AB3 the molecular shape is __________. -tetrahedral -trigonal planar, trigonal pyramidal, or T-shaped -linear, bent, or T-shaped -linear, bent, or trigonal planar -linear, octahedral, or bent

-Element x -Element y -Element Z (The inward "pull" on the electrons from the nucleus is called the effective nuclear charge. When looking at a series of atoms within the same period, the greater the pull on the electrons, the smaller the atom and the harder it is to remove an electron.)

For the series of elements X, Y, and Z all in the same period (row), arrange the elements in order of decreasing first ionization energy. (High to low)

Which noble gas has the highest first ionization energy?

He

Which noble gas has the highest first ionization energy? (opposite to atomic radius)

He

c= λ × ν (c - the speed of light)

How are the wavelength (λ) and frequency (ν) of light related? -c= λ × ν (c - the speed of light) -c= ν / λ (c - the speed of light)

Rank N₂, H₂, and CO₂ in increasing bond order?

H₂ CO₂ N₂

Predict if a bond between two atoms is nonpolar covalent, polar covalent, or ionic. (test objective)*

If the difference of the electronegativity between the two elements is greater than 1.7 then the bond is ionic. The difference with a polar covalent bond is 0.4 to 1.8 and a nonpolar covalent bond is from 0 to 0.4.

the atomic radii

In the space-filling model, what determines the relative sizes of the spheres? -the number of bonds -the type of atoms -the atomic radii -the bond length

Which atom has the highest electronegativity? K or Rb?

K-0.73 (Rb=0.71)

_______ _______ are based on the number of valence electrons present in each of the constituent atoms of the molecule

Lewis Structures

Of the atoms below, ____ is the most electronegative

Li

Which element has the lowest electronegativity? -C -Li -N -O -F

Li

Rank the following elements in order of decreasing atomic radius. B. Li, N, Be

Li, Be, B, N (they are in the same period, so is decreases moving from left to right.

The element that corresponds to the electron configuration 1s², 2s², 2p⁶, 3s² is __________. -sodium -neon -fluorine -magnesium

Magnesium

Which has the highest electronegativity? Na, Mg, K, Ca.

Mg

Of the following atoms, which has the largest first ionization energy? -P -B -N -C -Si

N

Which element has the lowest ionization energy? -P -Cl -Si -Mg -Na

Na

Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? -Na > Mg > Si > P > Ar -Ar > Si > P > Na > Mg -Mg > Na > P > Si > Ar

Na > Mg > Si > P > Ar

Which two elements have the same ground-state electron configuration? -Cu and Ag -Fe and Cu -Cl and Ar -Pd and Pt -No two elements have the same ground-state electron configuration.

No two elements have the same ground-state electron configuration.

Which set has the correct order of decreasing first ionization energy? -O < Br < Ba < Mg -O > Br > Mg > Ba -O < Mg < Br < Ba

O > Br > Mg > Ba

In which set of elements would all members be expected to have very similar chemical properties? -O, S, Se -Na, Mg, K -S, Se, Si -N, O, F -Ne, Na, Mg

O, S, Se

Which one of the following has the smallest radius? -Al -Mg -Ca -P

P

Which equation correctly represents the first ionization of phosphorus? =P(g)→P+(g)+e− =P+(g)+e−→P(g) =P(g)→P−(g)+e−

P(g)→P+(g)+e−

Which element has the largest atomic radius? (quiz) -K -He -Rb -Xe -all have the same radius

Rb

Rank the following elements in order of decreasing atomic radius. K, Rb, Li, Na

Rb, K, Na, Li (TIP: Atomic radii increase going down a group, because successively larger valence-shell orbitals are occupied by electrons. For example, rubidium has electrons in the fifth shell, which contains much larger orbitals than the fourth, third, second, or first shells.)

Which element would have 4d^6 as the last entry of its electron configuration (quiz) -Fe -Kr -Ru -Xe

Ru

Of the following atoms, which has the largest first ionization energy? -As -Sb -Ge -Se -S

S (16)

Three monosulfur fluorides are observed: SF2, SF4, and SF6. Of these, __________ is/are polar.

SF2 and SF4 only

(Quiz) Which element has this excited natural state electron configuration? [Ar]3d¹⁰, 4s¹, 5s¹ -Br -Cs -Ga -Rb -Se

Se

Arrange the elements in decreasing order of first ionization energy. Rank from highest to lowest first ionization energy.

Se, Ge, In, Cs

gas, liquid, solid (test objective)

Solid-least amount of energy (compact, tight) liquid-(have more energy than a solid b/c the molecules has wiggle room) gas-greatest amount of energy (free, lots of room)

Bond order, bond length, and bond energy are closely related. The shorter a bond, the _____ its bond strength. A shorter bond will therefore have a higher energy than a longer bond. Bond order also plays a role. For a given pair of atoms, the higher the bond order, the shorter and ______ the bond will be.

Stronger, Stronger

What is the molecular geometry of a molecule with 3 outer atoms and 2 lone pairs on the central atom? Enter the molecular geometry of the molecule.

T-shaped

Even though H has only one electron, there are many lines in the atomic spectrum of H. Explain** -There are several other particles within the H atom -There are many energy levels within the H atom -Different lines are generated by different H atoms -There is no explanation yet.

There are many energy levels within the H atom

The molecular geometry of the BrO3 - ion is __________. -T shaped -Trigonal pyramidal -trigonal planar -tetrahedral -bent

Trigonal pyramidal

This is a violation of Hund's rule T/F 1s ↑↓ 2s ↑↓ 2p↑↓ _ _

True

This is a violation of Hund's rule T/F 1s↑↓ 2s↑↓ 2p ↑ ↑↓ _

True

True or False: The shorter the bond, the stronger the bond is

True

Which is true about the actinides? -Uranium is an example of an actinide element -Actinides are built up by filling the 4f orbitals -Most of the actinides are found in nature -Actinides are often referred to as the rare earth elements.

Uranium is an example of an actinide element.

Non-Polar Bonds

When atoms or similar electronegativities share electrons to form a covalent bond, the shared electrons tend to be evenly controlled by both atoms (a covalent bond in which electrons are shared equally)

1s-↑↑ 2s-↑↓ 2p _ _ _

Which is a violation of Pauli exclusion principle?

Octahedral

Which of these molecular shapes do you expect for the SF6 molecule? -linear -trigonal planar -tetrahedral -trigonal bipyramidal -octahedral

yes

Would the molecule have a nonzero dipole moment? yes or no

Which element would be expected to have chemical and physical properties closest to those of krypton? (trends) -Te -As -At -Xe -Ge

Xe

The condensed electron configuration of krypton, element 36, is -[Ar] 3d¹⁰, 4s², 4p⁶ -[Ar] 4s⁴, 3d⁴ -[Ar] 4s⁴

[Ar] 3d¹⁰, 4s², 4p⁶

Write the condensed electron configurations for the Ca atom.

[Ar]4s^2

Write the condensed electron configuration for Ga (^)

[Ar]4s^2, 3d^10, 4p^1

The ground state (condensed) electron configuration for Zn is_______ -[Kr]4s^2, 3d^10 -[Ar]4s² 3d¹⁰ -[Ar] 4s¹ 3d¹⁰

[Ar]4s² 3d¹⁰

The ground state configuration of fluorine is __________. (normal) -[He] 2s², 2p² -[He]2s², 2p⁵ -[He]2s², 2p³

[He]2s², 2p⁵

What is the condensed electron configuration of Iodine

[Kr]5s^2, 4d^10, 5p^5

First ionization energy

_____ _______ ______ refers to the energy required to remove an electron from an electrically neutral atom in the gas phase.

All of the __________ have a valence shell electron configuration ns¹ -halogens -noble gases -alkali earth metals -alkali metals

alkali metals

Write the Lewis Structure for PCl₃ (quiz question)

all follow the octet rule

Elements in the modern version of the periodic table are arranged in order of increasing __________.

atomic number

The molecular geometry of the SF2 molecule is __________. -tetrahedral -octahedral -trigonal planar -bent -linear

bent

What is the molecular geometry of a molecule with 2 outer atoms and 2 lone pairs on the central atom? Enter the molecular geometry of the molecule.

bent (tetrahedral)

When comparing orange light and blue light, the one with the greater energy is -orange light -blue light -infrared light -ultraviolet light

blue light

Are frequency and wavelength AND wavelength and energy inversely or directly proportional?

both inversely related

In counting the electron domains around the central atom in VSEPR theory, a __________ is not included. -nonbonding pair of electrons -double covalent bond -single covalent bond -core level electron pair -triple covalent bond

core level electron pair

Hund's rule

describes how electrons are distributed among orbitals of the same sublevel when there is more than one way to distribute them. -All orbitals in the same sublevel have one electron -They all have the same spin

Pauli exclusion principle

describes the restrictions on the placement of electrons into the same orbital. If 2 electrons occupy the same orbital, they have to have opposite spins

Are energy and frequency inversely or directly proportional?

directly proportional

Which bond is shorter, a double bond or single bond?

double bond

The basis of the VSEPR model of molecular bonding is __________.

electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions (as far apart as possible)

The number of electromagnetic waves that travel past a certain point in a given time is the ________ of the radiation.

frequency

What are the D-block elements (what groups)

groups 3-12 (transitions metals)

elements with the valence-shell electron configuration ns² np⁵ is what in the periodic table (name group)

halogens

The ____ the bond order means the ___ it is to break

higher, harder

The ____ the bond order, the ___ bond energy is required

higher, more

Lewis Dot structure video -explanation -steps -how to figure out valence electrons -drawing structure

https://youtu.be/cIuXl7o6mAw

Atomic emission spectra are due to electrons____________. -Atomic emission spectra are due to electrons in an atom rising from one energy level to a higher one -being added to an atom -changing state from solid to liquid -in an atom dropping from one energy level to a lower one

in an atom dropping from one energy level to a lower one

As bond length ____, bond energy _____.

increase, decreases

The first ionization energies of the elements __________ as you go from left to right across a period of the periodic table, and __________ as you go from the bottom to the top of a group in the table.

increase, increase

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

increases, decreases

The molecular geometry of the CS2 molecule is __________. -tetrahedral -linear -bent -T-shaped -trigonal planar

linear

For a molecule with the formula AB2, the molecular shape is __________. -trigonal planar -linear or T-shaped -T-shaped -linear or trigonal planar -linear or bent

linear or bent

The molecular geometry of the BeCl2 molecule is _______, and this molecule is_____. -linear, polar -linear, nonpolar -bent, polar -bent, nonpolar -trigonal planar, polar

linear, nonpolar

_____ are created when atoms are combined together

molecules

When ultraviolet energy is absorbed by an atom, an electron____. -moves from a lower to a higher energy level -moves from a higher to a lower energy level

moves from a lower to a higher energy level

is CCl4 polar or nonpolar

nonpolar

is XeF4 nonpolar or polar

nonpolar

zero dipole moment

nonpolar

Which shape in the figure could lead to a square-planar shape upon removal of one or more atoms? -linear -trigonal planar -tetrahedral -trigonal bipyramidal -octahedral

octahedral

The molecular geometry of the SF6 molecule is __________, and this molecule is __________. -trigonal pyramidal, polar -trigonal bipyramidal, polar -trigonal planar, polar -octahedral, nonpolar -trigonal planar, nonpolar

octahedral, nonpolar

When comparing orange light and infrared light, the one with the greater energy is______. -orange light -blue light -infrared light -ultraviolet light

orange light

ultraviolet light

part of the electromagnetic spectrum that consists of waves with frequencies higher than those of visible light and lower than those of x-rays

The smallest particle of light is called a ________. -packet -photon -frequency

photon

is SF4 nonpolar or polar

polar

nonzero dipole moment

polar

Bonds that are partly ionic are called

polar covalent bonds

Infrared radiation has a shorter wavelength than ________. -Ultraviolet -Visible light -radio waves -Microwaves

radio waves

What have the longest wavelengths (lower energy

radio waves (KNOW THIS PICTURE)

What is the Lewis structure for Iodine

seven dots around an I

covalent bonds

sharing of two electrons in the valence shell of both atoms

the formal charge of each atom is calculated by:

subtracting the number of valence electrons assigned to the atom from the number of valence electrons in diagram

(quiz) What is the molecular shape of methane, CCl4? -bent -linear -trigonal planar -tetrahedral

tetrahedral

The molecular geometry of the CHCl3 molecule is __________. -trigonal planar -tetrahedral -T-shaped

tetrahedral

The molecular geometry of the CHF3 molecule is __________, and the molecule is __________. -seesaw, nonpolar -seesaw, polar -tetrahedral, polar -tetrahedral, nonpolar -trigonal pyramidal, polar

tetrahedral, polar

What is the lewis structure for H₃CH? Is the C-H bond stronger than a Si-H bond

the C-H bond is stronger because it is smaller (it's above the Si)

Ionization energy is: -the energy required to add an electron to the ground state of a neutral gaseous atom or ion. -the energy released when an electron is added to the ground state of a neutral gaseous atom or ion. -the energy released when two ions come together. -the energy required to remove an electron from the ground state of a neutral gaseous atom or ion.

the energy required to remove an electron from the ground state of a neutral gaseous atom or ion.

Which statement best describes the polarity of CF2I2? -The molecule is always polar. -The molecule is always nonpolar. -Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar.

the molecule is always polar

What do the group numbers from 1A to 8A for the elements indicate about the electrons configurations of those elements -total number of protons -the number of valence electrons -the number of energy sublevels -total number of electrons

the number of valence electrons

The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell, element X has a partially filled 4d subshell. What type of element is X? -transition metal -alkali metal -halogen -main group element -chalcogen

transition metal

According to VSEPR theory, if there are three electron domains in the valence shell of an atom, they will be arranged in a(n) __________ geometry. (test objective)

trigonal planar

The molecular geometry of the BCl3 molecule is __________, and this molecule is __________. -trigonal pyramidal, polar -trigonal planar, polar -trigonal bipyramidal, polar -trigonal pyramidal, nonpolar -trigonal planar, nonpolar

trigonal planar, nonpolar

The molecular geometry of the PHCl2 molecule is __________. -trigonal planar -bent -trigonal pyramidal -tetrahedral -T-shaped

trigonal pyramidal

What is the molecular geometry of a molecule with 3 outer atoms and 1 lone pair on the central atom? Enter the molecular geometry of the molecule.

trigonal pyramidal

The molecular geometry of the PF3 molecule is __________, and this molecule is __________. -trigonal planar, polar -trigonal pyramidal, polar -tetrahedral, unipolar -trigonal pyramidal, nonpolar -trigonal planar, nonpolar

trigonal pyramidal, polar

What bond would be harder to break? one with a triple bond or one with a double bond?

triple bond

Which has a higher energy? -infrared radiation -ultraviolet radiation

ultraviolet radiation

All electromagnetic radiation travels at the same ________. -velocity -energy -wavelength -frequency -color

velocity

Electromagnetic radiation normally travels in the form of ________. -waves -beats -seconds

waves

Can ultraviolet light be used as a treatment for certain cancers? (yes/no)

yes