Sem 1- 6 week (2) Flashcards by celine obeid

What was the most important finding in Rutherford’s gold foil experiment?
Electrons orbit the nucleus at specific energy levels.
Protons and neutrons are found in the nucleus of the atom.
Atoms are mostly empty space but not completely empty.
Electrons have a negative charge and protons have a positive charge.

Atoms are mostly empty space but not completely empty.

How well did you know this?

Not at all

Perfectly

Based on our current understanding of the atom, electrons orbit the nucleus of the atom at specific energy levels.
True
False

False

How well did you know this?

Not at all

Perfectly

Which of the following scientists was the first to make observations that showed that atoms existed?
  Democritus 
  Rutherford 
  Thomson 
  Dalton

Dalton

How well did you know this?

Not at all

Perfectly

Where are the electrons found within the atom?

Electrons are found outside of the nucleus.

How well did you know this?

Not at all

Perfectly

Where are the protons found within the atom?

Protons are found in the nucleus.

How well did you know this?

Not at all

Perfectly

When Thomson performed his cathode ray tube experiment, he found that the beam of gas was attracted to the positively charged plate. If he had found that the beam of gas was attracted to the negatively charged plate, which particle would he have found?
  The proton. 
  The neutron. 
  The electron. 
  The nucleus.

The proton.

How well did you know this?

Not at all

Perfectly

How many protons does chlorine, Cl, have?

How well did you know this?

Not at all

Perfectly

What is the mass number of an atom that has 15 protons and 16 neutrons?
  15 
  16 
  31 
  30.97

How well did you know this?

Not at all

Perfectly

Write the isotope notation for an atom that has 7 protons and 9 neutrons.

Nitrogen-16

How well did you know this?

Not at all

Perfectly

If 15% of the atoms of a certain element have a mass of 14.00 amu and 85% of the atoms have a mass of 15.00 amu, then the average atomic mass is 14.50 amu.
True
False

False

How well did you know this?

Not at all

Perfectly

Which of the following would the average atomic mass be closest to given the following information?

Isotope Mass (amu) Isotope Abundance (%)

00 65.74
00 34.26
00
00
00
00

18.00

How well did you know this?

Not at all

Perfectly

An element has three isotopes. The first isotope (4.00 amu) has an abundance of 87.46 %, the second isotope (5.00 amu) has an abundance of 11.57 %, and the third isotope (6.00 amu) makes up the remainder of the abundance. What is the average atomic mass of the element?

66 amu
08 amu
14 amu
00 amu

4.14 amu

How well did you know this?

Not at all

Perfectly

In a sample of 200 atoms, 195 are atoms (97.50 % of the total atoms) with a mass of 14.00 amu and 5 atoms (2.50 % of the total atoms) with a mass of 15.00 amu. What is the average atomic mass of this sample? (Be sure to show your work!)

14.03 amu

How well did you know this?

Not at all

Perfectly

One of nitrogen’s isotopes has a mass number of 15. How many neutrons are in the nucleus of this isotope?

Nitrogen- 15

Protons- 7

15-7= 8 Neutrons

How well did you know this?

Not at all

Perfectly

(460-370 BCE) A Greek philosopher who theorized that all matter could be reduced to particles that could not be divided, which he described as “atomos.”

Democritus

How well did you know this?

Not at all

Perfectly

everything is made up of atoms
atoms are invisible and smallest part of matter
all atoms have same element mass and shape
atoms can’t be created or destroyed
atoms can be combined to make compounds

John Dalton

How well did you know this?

Not at all

Perfectly

did an experiment on how atoms are made up of other components
used cathode ray
discovered the electron

JJ Thomson

How well did you know this?

Not at all

Perfectly

used gold and alpha, the alpha bounced back b/c of nucleus

- discovered nucleus

Ernest Rutherford

How well did you know this?

Not at all

Perfectly

energy levels

- electrons have energy which keeps them in orbit but they are still attracted to (+)

Bohr

How well did you know this?

Not at all

Perfectly

electron cloud model

- used BOHR MODEL & math to calculate the probabiltity of finding electrons

Erwin Schrodinger

How well did you know this?

Not at all

Perfectly

An isotope with 7 protons and 8 neutrons would have which of the following isotope notations?
  P - 15 
  N - 7 
  N - 15 
  O - 15

N - 15

How well did you know this?

Not at all

Perfectly

Use the following information below to calculate the average atomic mass. Be sure to show your work.

Isotopic Mass Number Relative Abundance
28 66.28%
29 26.34%
30 7.38%

28.41 amu

How well did you know this?

Not at all

Perfectly

Which of the following was not a conclusion from Rutherford’s experiments with gold foil?

The atom is mostly empty space with a small, solid center.
Electrons are outside the nucleus at very specific energy levels.
The protons are in the nucleus of the atom and electrons are outside the nucleus.
There is a tiny nucleus within the atom.

Electrons are outside the nucleus at very specific energy levels.

How well did you know this?

Not at all

Perfectly

Which element has the following electron configuration?

1s22s22p63s1

Lithium, Li
Magnesium, Mg
Sodium, Na
Neon, Ne

Sodium, Na

How well did you know this?

Not at all

Perfectly

``` How many electrons are in the third energy level for Zirconium, Zr? 2 8 10 18 ```

Which of the following is the electron configuration for Cesium, Cs? A. 1s22s22p63s23p64s23d104p65s25d105p66s1 B. 1s22s22p63s23p64s23d104p65s24d105p66s1 C. 1s22s22p63s23p64s24d104p65s25d105p66s1 D. 1s21p62s22p63s23p64s23d104p65s24d105p66s1 Choice A Choice B Choice C Choice D

Choice B

``` To write the shorthand configuration for Oxygen, O, which element would you put in brackets? Helium, He Oxygen, O Neon, Ne Lithium, Li ```

Helium, He

``` The following shorthand configuration belongs to which element? [Kr]5s24d105p5 Bromine, Br Iodine, I Chlorine, Cl Krypton, Kr ```

Iodine, I

1s22s22p63s23p64s1 is the electron configuration for which element?

Potassium

When writing the shorthand notation for sulfur, S, which element would you put in brackets?

Neon [Ne]

How many valence electrons does indium, In, have?

1s22s22p63s23p64s23d1 is the electron configuration for which element?

Scandium

``` Which of the following is NOT shown in an electron configuration? The number of electrons. The spin of the electrons. The energy levels. The sublevels. ```

The spin of the electrons.

Write Selenium's electron configuration and use it to determine how many valence electrons it has.

1s^2^2s2^2p^63s^23p^64s^23d^104p^4 The outermost level is the 4th energy level, and there are 2 electrons in the s orbital and 4 electrons in the p orbital for a total of 6 Valence electrons

Write the electron configuration for Arsenic.

1s^22s^22p^63s^23p^64s^23d^104p^3

Write the electron configuration for silver.

1s^22s^22p^63s^23p^64s^23d^104p^65s^24d^9

``` Which of the following elements would have three valence electrons? Calcium, Ca Copper, Cu Gallium, Ga Sulfur, S ```

Gallium, Ga

``` Which of the following is not considered electromagnetic radiation? Visible light Gamma rays Sound waves Infrared waves ```

Sound waves

``` When the energy increases, which of the following decreases? Frequency Speed of light Wavelength Planck's constant ```

Wavelength

``` The height of a wave is referred to as the _____. wavelength amplitude trough frequency ```

amplitude

If a t-shirt looks in green in color, which of the following is correct? - The atoms in the dye that the t-shirt is made out of gives off green light. - The t-shirt absorbs only green light and emits only red light. - The t-shirt absorbs only red light and emits only green light. - The t-shirt absorbs every color of light except for green light.

The t-shirt absorbs every color of light except for green light.

The more waves that pass a point in a given amount of time means they have a longer wavelength. True False

False

How much energy does a wave with a frequency of 3.78 x 1010 Hz have?

2.51 x 10^-23 J

``` In a vacuum, all light waves ______. have the same wavelength. have the same energy. have the same speed. have the same frequency. ```

have the same speed.

The energy of a photon is 2.39 x 10-15 J. Calculate the wavelength. A. 1.20 · 1010 m B. 8.32 · 10-11 m C. 3.60 · 1018 m D. 2.77 · 10-19 m Choice A Choice B Choice C Choice D

Choice B

When an electron absorbs heat and then produces light, what happened to it? - The electron vibrates a little within the same energy level. - The electron drops an energy level. - The electron drops down an energy level and then back up an energy level. - The electron jumps up an energy level and then drops down an energy level.

The electron jumps up an energy level and then drops down an energy level.

The reason that electrons can absorb light energy is because light not only moves in waves, but also acts like matter that are called photons. True False

True

Knowing the relationship between energy and frequency and the equation that relates the two, what is the relationship between x and y in the following equation? x = (28)y Inverse Direct x = y There is no correlation between x and y

Direct

A wave of green light has a wavelength of 505 nm. How much energy does this wave have? Be sure to show your work! (Remember that 1 nm = 1⋅10^-9 m.)

3.94 x 10^-19 J

Photon A has a frequency of 5 waves per second and photon B has a frequency of 1 wave per second. Which photon will have the greatest wavelength? Explain how you know.

Photon B has a longer wavelength. Light with a longer wavelength has a lower frequency.

The frequency of a wave is 4.28 · 1020 Hz. How much energy does this wave have? Be sure to show your work!

2.84 · 10^-13 J

``` The amount of energy that an electron has normally is best referred to as its ______. frequency wavelength excited state ground state ```

ground state

The energy of a photon is 6.43 · 10-14 J. What is the wavelength? Be sure to show your work!

3.09 · 10^-12 m

The scientist that created the Periodic Table is ________________.

Mendeleev first created the Periodic Table.

Mendeleev organized the elements on the Periodic Table by increasing __________________.

atomic mass or weight

The modern Periodic Table has elements arranged in order of increasing atomic mass. True False

False

``` Sodium is a metal that reacts violently when exposed to water. Which other element do you expect to react violently when exposed to water? Magnesium Aluminum Cesium Chlorine ```

Cesium

Phosphorous is located in period 3 and group 15. True False

True

``` Mendeleev organized elements in the Periodic Table by _______________________ while Mosley used ___________________________. Atomic mass, atomic number Atomic mass, atomic radius Atomic number, atomic mass Atomic number, atomic radius ```

Atomic mass, atomic number

``` How are elements in a period on the modern Periodic Table arranged? By chemical properties By physical properties By increasing number of protons By number of valence electrons ```

By increasing number of protons

``` What element is in Period 4 Group 17? Chlorine Iodine Actinium Bromine ```

Bromine

``` Nitrogen can be found in Period ________ and Group ________? 15, 2 2, 15 2, 7 7, 2 ```

2, 15

``` Groups ________ and _______contain elements whose valence electrons are only found in the s block? 17, 18 13, 14 1, 2 7, 8 ```

1, 2

``` The properties of elements reoccur periodically, demonstrating periodic trends when the elements are arranged in order of increasing reactivity atomic radius atomic mass atomic number ```

atomic number

Even though elements like Na, Li, K, and Ca, Mg, Ba share some similarities, why are they grouped into different families on the Periodic Table? They have different numbers of protons. They have different chemical properties They have different masses. They were discovered at different times.

They have different chemical properties

``` Argon is a gas at room temperature and has a very stable electron configuration. Which of the following elements would you expect to be gaseous and stable at room temperature? Chlorine Nitrogen Oxygen Neon ```

Neon

``` What do all members of a group have in common? Atomic mass Atomic number Atomic radius Valence electrons ```

Valence electrons

``` The halogen in Period 5 is ________. Fluorine Iodine Strontium Xenon ```

Iodine

``` Which element is the most reactive alkali metal? Magnesium Calcium Sodium Potassium ```

Potassium

``` Which element would be the worst conductor of electricity? Boron Aluminum Silicon Phosphorous ```

Phosphorous

Nonmetals tend to gain electrons to form negative ions. True False

True

``` Which family is most likely to form ions with a +1 charge? Alkali metals Alkaline earth metals Halogens Noble gases ```

Alkali metals

Why do elements in the same group share the same chemical properties? They have the same number of protons The valance electrons are in the same energy level They have the same number of valence electrons. They share the same physical properties

They have the same number of valence electrons.

``` Name the alkaline earth metal in period 7. Radium Francium Barium Radon ```

Radium

Why are noble gases unreactive? Because of the number of protons in the nucleus. Because they have a full valence shell of electrons. Because they are colorless and odorless gases. Because they need too many valence electrons to have a full shell.

Because they have a full valence shell of electrons.

``` Metals tend to ________ electrons to form a ________ ion. Gain, positive Gain, negative Lose, positive Lose, negative ```

Lose, positive

``` What are the most reactive metals on the periodic table? Transition metals Alkaline earth metals Rare earth metals Alkali metals ```

Alkali metals

``` What family contains the most chemically active non-metals? The oxygen family The carbon family The halogens The Noble gases ```

The halogens

Properties Element J Color Gray Reactivity Medium-low Phase of matter at room temperature Solid To which family might the element described above belong? Alkali metals Transition metals Halogens Noble gases

Transition metals

``` Alkali metals tend to form ions with what charge? +1 +2 -1 -2 ```

``` Nonmetals tend to _________ electrons and form _______ ions. Gain, positive Gain, negative Lose, positive Lose, negative ```

Gain, negative

``` Halogens tend to form ions with what charge? +1 +2 -1 -2 ```

-1

Which atom has a larger radius? Ca Se

Which atom has a larger radius? Oxygen Sulfur

Sulfur

Put the following elements in order of increasing atomic radius: Li, N, P, Cl Use commas to separate the elements.

Cl, N, P, Li

Why does Br have a smaller radius than K even though it has more protons and electrons? Because Br has fewer electron shells than K. Because Br has more electron shells than K. Because Br has a stronger nuclear charge than K Because Br has a weaker nuclear charge than K.

Because Br has a stronger nuclear charge than K

Why does electron shielding have very little effect on the size of the radius as you move across a period? Because the increase in the effective nuclear charge cancels out the effect of shielding. Because across a period, electrons are in the same shell so they experience very little shielding.

Because across a period, electrons are in the same shell so they experience very little shielding.

Which group of elements, metals or nonmetals, will tend to form ions that are larger than their parent atom? Metals Nonmetals

Nonmetals

Thinking about the size of the parent atom, which ion do you predict will be larger: Na1+ or K1+? K1+ Na1+

K1+

``` Which of the following atoms will form an ion that is smaller than its neutral atom? S O Li Ne ```

``` Choose the atom below that will form an ion that is larger than its neutral atom. Iron Copper Strontium Phosphorous ```

Phosphorous

List the following ions in order of increasing size: Ca2+, Na1+, S2-, Cl1- Use the names of the elements and commas to complete your answer.

Na1+, Ca2+, Cl1-, S2-

List the following atoms in order of decreasing electronegativity: Sr, Mg, Ca, Be, Ba Use the symbol with a comma in between each element to record your answer.

Be, Mg, Ca, Sr, Ba

Oxygen has a lower electronegativity than nitrogen. True False

False

``` Which atom is most likely to attract electrons in a bond? Al Si P S ```

Why is the electronegativity of a noble gas listed as zero? - The nuclear charge in the noble gases is so strong they do not attract electrons in a bond. - The nuclear charge in the noble gases is so weak they do not attract electrons in a bond. - Because noble gases do not typically participate in chemical bonds, they do not attract electrons when bonding. - Because noble gases will only attract electrons during a bond with other noble gases.

Because noble gases do not typically participate in chemical bonds, they do not attract electrons when bonding.

Using a drawing, compare the atomic radius of the following elements. Be sure your drawing ranks them from smallest radius to largest radius. Potassium Sodium Sulfur Selenium

Drawing should show the ranking from smallest to largest: Sulfur, selenium, sodium, potassium

What is the most important factor in determining a trend from left to right across a period? The strength of the nuclear charge The number of valence electrons The strength of the electron shielding The number of energy levels in the atom

The strength of the nuclear charge

___________ have low ionization energies because ____________. - Alkali metals; they have the weakest effective nuclear charge in a period. - Alkaline earth metals; they have highest electronegativities in the period. - Halogens; they have the weakest effective nuclear charge in a period. - Noble gases; they have the highest electronegativities in the period.

Alkali metals; they have the weakest effective nuclear charge in a period.

Consider atoms of oxygen and fluorine. Which atom will be the least likely to lose an electron to form an ion and why?

Fluorine because it has the stronger nuclear charge.

What is the most important factor in determining a trend from top to bottom in a group? The number of valence electrons The distance between the valence electrons and the nucleus The number of neutrons in the nucleus Whether the group consists of metals or nonmetals

The distance between the valence electrons and the nucleus

Explain the relationship between the size of an atoms’ radius and its ionization energy as you down a group from Na to Fr. (Hint: use the words increases and/or decreases.)

As the radius increases, the ionization energy decreases.

``` Which atom is most likely to attract electrons in a bond? K Na S Se ```

``` Which of the following atoms will form an ion with a radius larger than that of its neutral atom? Ca Mg Al O ```

Explain why cations tend to form ions with radii smaller than their neutral atom.

When they lose valence electrons, it increases the effective nuclear charge.

In any given period, which family will experience the strongest effective nuclear charge and why? - Alkali metals because they have the fewest number of protons. - Alkali metals because they have the most number of protons. - Halogens because they have the fewest number of protons. - Halogens because they have the most number of protons.

Halogens because they have the most number of protons.

``` What is the oxidation number of calcium? 1+ 2+ 3+ 4+ ```

``` An ion found in some compounds contains 12 protons and 10 electrons. What is its symbol? Ne Ne2- Mg2+ Mg+ ```

Mg2+

``` What type of compound is CHCl3, the anesthetic chloroform? Ionic Covalent Metallic Basic ```

Covalent

Which of the following substances would not conduct electricity in any state? One in which electrons are delocalised and shared among positive nuclei One in which electrons are transferred between ions One in which electrons are shared One in which electrons are kept and no ions are formed

One in which electrons are shared

``` What type of compound is Fe2O3, and what is its name? Covalent, diiron trioxide Acid, ferrous acid Base, iron hydroxide Ionic, iron(III) oxide ```

Ionic, iron(III) oxide

``` What is the name of the following compound, which contains a polyatomic ion: BeCrO₄? Beryllium chromate Beryllium chromium tetraoxide Beryllium oxide Beryllium dichromate ```

Beryllium chromate

``` What type of compound is CO2? Ionic Acid Base Covalent ```

Covalent

``` What is the name of the following compound, which contains a metal that can exhibit more than one ionic charge: PbCl2? Lead(II) Chloride Lead Chloride Lead(I) Chloride Lead Chloride(II) ```

Lead(II) Chloride

``` What is the name of the following compound, which contains a polyatomic ion: MgSO4? Magnesium sulfur oxide Magnesium sulfur tetraoxide Magnesium sulfate Magnesium oxide ```

Magnesium sulfate

``` What is the name of the following compound: XeF4? Monoxenon quadrafluorine Xenon tetrafluorine Monoxenon fluoride Xenon tetrafluoride ```

Xenon tetrafluoride

``` What is the name of the following compound: HCl? Hydrochloric acid Hydrogen chloride Monohydrogen monochloride Hydrogen(I) chloride ```

Hydrochloric acid

``` What is the name for the following compound: RbOH? Monorubidium hydroxide Monorubidium oxygen hydride Rubidium hydroxide Rubidium oxygen hydride ```

Rubidium hydroxide

``` What type of compound is TiCl4 and what is its name? Ionic, titanium(IV) chloride Covalent, titanium tetrachloride Acid, titanium chloric acid Base, titanium chloroxide ```

Ionic, titanium(IV) chloride

``` How many oxygen atoms are in the correct formula the ionic compound formed by the lithium cation, Li+, and the oxygen anion, O2−? 1 2 3 4 ```

``` How many nitrogen atoms are in the correct formula for the ionic compound calcium nitride? 1 2 3 4 ```

``` How many sodium atoms are in the correct formula for the ionic compound sodium chlorate? 4 3 2 1 ```

``` How many copper atoms are in the correct formula for the compound copper(I) oxide? 4 3 2 1 ```

``` How many hydrogen atoms are in the correct formula for hydrobromic acid? 4 3 2 1 ```

``` How many hydrogen atoms are in the correct formula for carbonic acid? 1 2 3 4 ```

``` How many oxygen atoms are in the correct formula for barium nitrate? 2 3 5 6 ```

``` How many oxygen atoms are in the correct formula for the covalent compound xenon trioxide? 1 2 3 4 ```

``` How many arsenic atoms are in the correct formula for the compound diarsenic pentoxide? 1 2 3 4 ```

``` How many sulfur atoms are in the correct formula for the compound tetraphosphorus heptasulfide? 4 5 6 7 ```

``` How many bromine atoms are in the correct formula for the compound lead(IV) bromide? 4 3 2 1 ```

``` How many hydroxide ions are in the correct formula for the compound calcium hydroxide? 1 2 3 4 ```

``` How many calcium atoms are in the correct formula for calcium phosphide? 1 2 3 4 ```

``` How many calcium atoms are in the correct formula for calcium chloride? 1 2 3 4 ```

``` How many fluorine atoms are in the correct formula for hydrofluoric acid? 4 3 2 1 ```

Write the formula and determine how many sodium ions are in the correct formula for sodium chlorate.

NaClO3 1 sodium ion

Write the formula and determine how many oxygen atoms are in the correct formula for iron(II) chlorite.

Fe(ClO2)2 4 Oxygen atoms

``` What is the name of the following compound: K3N? Tripotassium nitrogen Potassium nitrate Tripotassium mononitride Potassium nitride ```

Potassium nitride

``` What is the name of the following compound: Cr(NO3)3? Chromium(III) nitrate Chromium trinitrate Chromic acid Chromium nitrate ```

Chromium(III) nitrate

What is the name of the following compound: N2O3?

Dinitrogen trioxide

What is the name of the following compound: Al(OH)3?

Aluminum hydroxide

What is the name of the following compound: CaCO3?

Calcium carbonate

``` How many electrons are transferred in the following compound: BaO? 1 2 3 4 ```

``` How many electrons are transferred in the following compound: AlCl3? 1 2 3 4 ```

``` How many electrons are transferred in the following compound: Al2S3? 6 5 4 3 ```

``` Which of the following compounds share electrons? NaCl CO CsF KBr ```

``` In the compound CO2, how many lone pairs are on the central atom? 0 1 2 3 ```

``` How many bonded pairs of electrons are there in the molecule NOCl? 2 3 4 5 ```

``` How many bonded pairs of electrons are there in the molecule O2? 4 3 2 1 ```

``` What charge does an arsenic ion exhibit? 1- 2- 3- 4- ```

``` What charge does a beryllium ion exhibit? 1+ 2+ 3+ 4+ ```

``` How many bonded pairs of electrons are there in the molecule HCCH? 5 4 3 2 ```

How are electrons arranged in metallic bonds? They are transferred between ions. They are shared between nonmetals. They are delocalized and free-floating. They are held tightly by their nuclei.

They are delocalized and free-floating.

``` Which is not a property of metals? Brittle Malleable Ductile Conductive ```

Brittle

Why do metals bend and not break? They are made from positive and negative ions. They share electrons in discrete bonds. They have metallic luster.

They share electrons in discrete bonds.

True or False: Metals are good conductors of heat and electricity. True False

True

True or False: Most metals are found to occur naturally in their uncombined states. True False

False

The ability to be stretched into long wires is a property of metals known as __________________.

Ductility

True or False: All metals have high melting points. True False

False

``` An elemental metal contains how many types of atoms? 1 2 3 4 ```

What is the shape of the OF2 molecule?

Bent

Which of the following molecules is paired incorrectly with its shape? Xenon difluoride – Linear Methane (carbon tetrahydride) – Tetrahedral Beryllium chloride – Bent Boron trifluoride – Trigonal planar

Beryllium chloride – Bent

Sem 1- 6 week (2) Flashcards

(161 cards)