I tried to find the place where you found the two statements, and I could not.
Absence of long-range forces
The first statement makes sense to me:
There are no intermolecular forces except during the collision between molecules.
The OpenStax Chemistry textbook, for example, has this statement:
Gases are composed of molecules that are in continuous motion, traveling in straight lines and changing direction only when they collide with other molecules or with the walls of a container.
Both statements say the same thing: there are no long-range forces acting on the particles.
Your second statement does not make sense to me, and I think it contains a typo.
Collisions between two molecules do not exert unattractive or repulsive forces.
The corresponding statement in the OpenStax Chemistry textbook is:
Gas molecules exert no attractive or repulsive forces on each other or the container walls; therefore, their collisions are elastic (do not involve a loss of energy).
This statement also does not make sense to me. If there are collisions, there are repulsive forces. The second part is a known component of kinetic theory. The particles can exchange kinetic energy, but the total kinetic energy is conserved (or more stringently, momentum is conserved).
What were they trying to say?
Two billiard balls hitting each other are a good model of an elastic collision. Two balls covered in velcro are not - they are sticky. So in that sense, you want an absence of attractive interactions so that particles don't stick together (and form a condensed phase). I am puzzled why they think repulsive short-range interactions are incompatible with elastic collisions. Even attractive interaction are compatible with elastic collisions when they are sufficiently weak that they break when the repulsive interactions push the particles apart after colliding.
How do molecules actually behave?
Molecules have attractive interactions at short range that turn repulsive when they come too close together, for example modeled by a Lennard-Jones potential for noble gas particles. A substance like water make hydrogen bonds at short range. Using water as a example, these interactions are not magically turn off when liquid water turns into a gas. Instead, they become negligible because the molecules have high kinetic energy (or for low pressure, the number of collisions decreases compared to normal pressure). So for a gas much hotter than its boiling point, we can neglect those interactions and still get a good explanation of the temperature vs. pressure behavior.