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Chemistry Final Flashcards

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1
Q

Which three groups of the periodic table contain the most elements classified as metalloids (semi metals) ?

A

14, 15, and 16

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2
Q

Which element has the highest first ionization energy ?

A

Phosphorus

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3
Q

When a metal atom combines with a nonmetal atom , the nonmetal atom will

A

Gain electrons and increase in size

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4
Q

Which of the following elements has the smallest radius ?

A

Nickel

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5
Q

Which element in group 15 has the strongest metallic character ?

A

Bi

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6
Q

When combining with nonmetallic atoms , metallic atoms generally will

A

Lose electrons and form positive ions

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7
Q

Atoms of elements in a group on the periodic table have similar chemical properties. The similarity is most closely related to the atoms

A

Number of valence electrons

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8
Q

As atoms of elements in group 16 are considered in order from top to bottom , the electronegativity of each successful element

A

Decreases

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9
Q

An atom of which of the following elements has the greatest ability to attract electrons

A

Nitrogen

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10
Q

When electrons in an excited state fall to lower energy levels , energy is

A

Released only

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11
Q

Which elements ionic radius is smaller than its atomic radius ?

A

Sodium

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12
Q

Which formula represents a molecular substance ?

A

CO

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13
Q

A strontium atom differs from a strontium ion in that the atom has a greater

A

Number of electrons

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14
Q

Which of the following is a binary compound ?

A

Hydrogen sulfide

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15
Q

What is the formula for sodium oxalate ?

A

Na2C2O4

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16
Q

Given the unbalanced equation: Al + O2 -> Al2O3 , when this equation is completely balanced using the smallest whole numbers , what is the sum of the coefficients ?

A

9

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17
Q

What is the empirical formula of the compound whose molecular formula is P4O10?

A

P2O5

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18
Q

What is the molar mass of K2CO3 ?

A

138 grams

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19
Q

A compound is 86% carbon and 14% hydrogen by mass. What is the empirical formula for this compound ?

A

CH2

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20
Q

As independent particles , most atoms are

A

at relatively high potential energy

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21
Q

A compound is

A

A pure substance that cannot be broken down into simpler , stable substances

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22
Q

Which properties are more typical of molecular compounds than of ionic compounds ? (Circle all that apply)

A
  • they are gasses or liquids at room temperature

* Atoms share electrons

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23
Q

Which of these choices is the electron configuration of the iron (III) ion ?

A

[Ar]4s23d3

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24
Q

Which of these species make an isoelectric pair : Cl- , O2- , F , Ca2+ , Fe3+

A

Cl- and Ca2+

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25
Q

Which of these compounds is most likely to be covalent ? (Circle all that apply)

A

NF3

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26
Q

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm?

A

246 kJ

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27
Q

Which one of the compounds below represents a product of the KOH and H2SO4

A

K2SO4

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28
Q

Which of these chemical equations describes a halogen displacement reaction?

A

2KBr(aq) + Cl2(g) -> 2KCl(aq) + Br2(l)

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29
Q

Calculate the mass of excess reagent remaining at the end of the reaction in which 90 grams of SO2 are mixed with 100 grams of O2 to produce SO3

A

77.6 grams

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30
Q

How many moles of NO2 are present in 114.95 grams

A

2.498 moles

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31
Q

What is the mass percentage of OH- in Ca(OH)2?

A

45.9%

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32
Q

A 10.64 gram sample of a phosphorus compound is analyzed and found to be made up of 9.65 grams of phosphorus and 0.99 grams of oxygen. The experimental molar mass was found to be 350 g/mol. What is the molecular formula of this compound ?

A

P10O2

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33
Q

When heated , a metal carbonate decomposes into and

A

A metal oxide and carbon dioxide

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34
Q

Group 1 metals react with water to produce

A

Metal hydroxides and hydrogen.

35
Q

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

A

Mendeleev

36
Q

The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic

A

Numbers

37
Q

Atoms of the same element with different mass numbers are called

A

Isotopes

38
Q

Which pair of elements would be most likely to form an ionic compound

A

F and Al

39
Q

The correct name for NH4NO3 is

A

Ammonium Nitrate

40
Q

The chemical formula for Iron (II) Nitrate is

A

Fe(No3)2

41
Q

The energy required to remove an electron from an atom is the atom’s

A

Ionization energy

42
Q

The percent yield for the reaction between phosphorus and tri-chloride and chlorine gas yielding phosphorus penta-chloride is 83.2% what mass of phosphorus penta-chloride is expected from the reaction of 73.7 grams of phosphorus trichloride and excess chlorine

A

93.6 grams

43
Q

The precipitate formed when barium chloride is treated with sulfuric acid is

A

BaSO4

44
Q

The atom having the valence shell configuration 4s24p5 would be in

A

Group VII and period 4

45
Q

Select the term best describing the series of elements : Mn, Fe, Co, Ni, Cu

A

Transition metals

46
Q

Which element has the largest atomic radius

A

Rb

47
Q

Which of the following terms accurately describes the energy associated with the process : Li (g) -> Li(g) + e

A

Ionization energy

48
Q

The species that contains 24 protons , 26 neutrons , and 22 electrons would be represented by the symbol

A

50Cr2+

49
Q

Which element has the lowest first ionization energy

A

Xe

50
Q

Which element has the highest first ionization energy ?

A

N

51
Q

Which of these isoelectronic species has the smallest radius

A

Sr2+

52
Q

Which of the following elements has the greatest attraction for electrons in a covalent bond

A

Br

53
Q

Which statement is wrong ?

A

A phosphorus atom is larger than an antimony atom

54
Q

All of the following properties of the alkaline earth metals increase going down the group except

A

First ionization energy

55
Q

Which of the following is an ionic hydride

A

KH

56
Q

How many moles of CO2 are present in 220 mg

A

0.005 mole

57
Q

What is the percent water in hydrated calcium chloride

A

24.51%

58
Q

What is the molecular formula for a compound that is 46.16% carbon , 5.16% hydrogen and 48.68% fluorine , if the molar mass of this compound is 156.12 grams

A

C6H8F4

59
Q

If 2.68 grams of hydrated sodium sulfate on heating produces 1.26 grams of water , what is the empirical formula of this compound ?

A

Na2SO4 ->7H2O

60
Q

One mole of (NH4)2HPO4 contains ____ moles of hydrogen atoms

A

9

61
Q

Which of the following conclusions can be drawn from J.J. Thompson’s cathode ray experiments ?

A

Atoms contain electrons

62
Q

In the periodic table , as the atomic number increases from 11 to 17 , what happens to the atomic radius ?

A

It decreases only

63
Q

Which of the following is a correct interpretation of the results of Rutherfords experiments in which gold atoms were bombarded with alpha particles ?

A

The positive charge of an atom is concentrated in a small region

64
Q

Which of the following represents a pair of isotopes

A

Atomic number : Atomic Mass
———————•——————
7. : 13.
7. : 14.

65
Q

Which of the following properties generally decreases across the periodic table from sodium to chlorine

A

Atomic radius

66
Q

The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of the following ?

A

Na has a higher neutron to proton ratio than Ne

67
Q

Propane gas burns in excess oxygen gas. When the equation for this reaction is correctly balanced and all coefficients are reduced to their lowest whole-number terms, the coefficient for O2 is……

A

5

68
Q

Consider the element with the electron configuration [Kr]5s2,4d10,5p5. The element is

A

Halogen

69
Q

How many electrons are in the 4p orbitals of vanadium

A

0

70
Q

Consider the following reaction : 3Li + Z -> Li3Z

What is the formula for the compound if we substitute magnesium for lithium

A

Mg3Z2

71
Q

What is the charge on the monatomic ion that calcium forms in its compounds ?

A

+2

72
Q

What is the wavelength of radiation that has a frequency of 6.912 X 10(14) s-1

A

4.337 X 10(2) nm

73
Q

Which of these solids would have the lowest melting point ?

A

KF

74
Q

Which of these chemical equations describes a precipitation reaction ?

A

CaBr2 + H2SO4 -> CASO4 + 2HBr

75
Q

Which of these elements is chemically similar to potassium ?

A

Cesium

76
Q

The correct name for KHCO3 is

A

Potassium hydrogen carbonate

77
Q

What is the empirical formula for a compound that is 31.9% potassium , 28.9% chlorine , and 39.2% oxygen

A

KCLO3

78
Q

A compound contains 259.2 grams of F and 40.8 grams of C and has an experimental molar mass of 176.02 grams/mol , what would be the molecular formula of this compound ?

A

C2F8

79
Q

The complete balanced equation for the reaction between zinc hydroxide and acetate acid is

A

Zn(OH)2 + 2CH3COOH [] Zn(CH3COO)2 + 2H20

80
Q

The person whose work lead to a periodic table based on increasing atomic number was

A

Moseley

81
Q

The most reactive group of non-metals is the

A

Halogens

82
Q

Compared to the alkali metals , the alkaline-earth metals

A

Are less reactive

83
Q

A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called

A

Electronegativity

84
Q

How does the energy required to remove an electron from an atom changes as you move left to right in period 4 from potassium through iron ?

A

It generally increase

Chemistry Final (1 decks)

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